parvpaigwar

How menstruation linked with ovulation?

Determine the equivalent acid-base equilibrium that results when each of the following pairs of solutions is mixed. 25.0 mL of 0.50 M NaOH + 12.0 mL of 1.50 M HCl Pick two initial conditions from first four choices. Pick one choice from remaining choices to indicate type of equivalent solution.Choose at least one answer. a. Weak acid b. Strong acid c. Weak base d. Strong base e. pH determined by excess concentration of diluted strong acid (some acid used to neutralize base) f. pH determined by excess concentration of diluted strong base g. pH determined by concentration of diluted strong acid h. pH determined by buffer equation (resulting mixture produces a buffer) i. pH determined by conjugate base concentration (equivalent to equivalence point in titration of weak acid) j. pH determined by excess concentration of diluted strong base (remaining strong base + weak conjugate base = beyond equivalence point in titration of weak acid)

IPA                                                Gloss

pəluqʰ                                      ‘ash’

iika                                           ‘my eye’

aŋutʰkʰ                                    ‘two men’ 

kaːnəkʰt͡ʃakʰ                            ‘something that looks like frost’

pistəŋuːtʰ                                ‘they are servants’ 

arnakʰ                                      ‘two women’ 

tuqmikʰ                                    ‘bucket, pail’

pʰki                                           ‘concerning travel’

arnaqʰ                                      ‘woman’

aŋutʰqʰ                                     ‘man’

aŋutʰtʰ                                      ‘three or more men’

aquqʰ                                       ‘middle finger’ 

plaːiinaqʰ                                  ‘string’ 

arnatʰ                                       ‘three or more women’

kuikʰ                                         ‘river’



1. List preceding and following environments for the sets of segments [p t k q] and for [pʰ tʰ kʰ qʰ].

[p t k q]

before:
after:

[pʰ tʰ kʰ qʰ]

before:
after:

2. These two classes of sounds are in complementary distribution. In a sentence or two, clearly state how you can tell that they’re in complementary distribution. Be as specific as possible.

3. Using features, characterize the environments where the alternation between plain and aspirated stops occurs. (One of the environments will be “elsewhere”.)

• [p t k q] occur:

• [pʰ tʰ kʰ qʰ] occur:

4. Using features, character the natural segment classes consisting of       [p t k q] and of [pʰ tʰ kʰ qʰ].

• [p t k q]:

• [pʰ tʰ kʰ qʰ]:

5. Write a rule (in formal notation) that describes the relationship between [p t k q] and [pʰ tʰ kʰ qʰ] in Central Alaskan Yup’ik.

6. Show derivations for the following surface forms.

UR

Rule

SR                 [aquqʰ]                 [aŋutʰkʰ]                 [tuqmikʰ]                 [pʰki]
 

After reading answer briefly answer the 3 questions. 

One of the oldest medications still used often in clinical practice is heparin. It was founded in 1916 before the Food and Drug Administration was created. Generated nearly solely from pigs' mucosal tissues. (Hedlund, 2013) The market for heparin depends on China because of its sizable swine herds. The drug's supply chain starts at slaughterhouses, then moves on to tiny workshops that collect heparin crude by removing the mucous membranes from pig intestines. Then, after being further refined into an active pharmaceutical component, the crude heparin is sold to other facilities, often via consolidators (API). In order to generate a completed heparin product, such as an injectable pharmaceutical vial, this API is then mixed with inactive components (typically a sterile solution). (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012)

The drug heparin was recalled on a global scale in 2008. Numerous fatalities and adverse events were found to be caused by a contaminate identified as oversulfated chondroitin sulphate, according to researchers. (Hedlund, 2013) 81 individuals died as a result of it.  Eventually, it was discovered what triggered the undesirable effect that resulted in the fatalities and injuries. The contaminated chemical was an over-sulfated derivative of chondroitin sulfate, a similarly comparable compound derived from animal or fish cartilage and frequently used as an arthritis therapy. Since over-sulphated chondroitin is not a naturally occurring molecule, it is not as expensive as actual heparin starting material, and it matches the in-vitro characteristics of heparin, the fake was very definitely made intentionally rather than by mistake during production. The contamination was caused by a combination of a lack of appropriate pigs in China and cost-effectiveness, also it was discovered that the raw heparin batches had been reduced by 2 to 60% with the fake chemical. (Chinese Heparin Manufacturer Again Involved in Falsification and GMP Non-Compliance - ECA Academy, 2016)

Following the adulteration, investigations revealed that OSCS was present in both the finished heparin API produced by SPL-CZ and the raw material sent to the firm by Chinese contractors. The specific source or suppliers of the heparin adulteration are still unknown to Baxter and the FDA; however, evidence shows that OSCS was most certainly introduced by organizations upstream of the Chinese API production facility, Scientific Protein Laboratories-Changzhou (SPL-CZ). Starting in 1996, Chinese raw materials have been used to make Baxter's heparin API; SPL-CZ joined the company's heparin production process in 2004. (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012)

The U.S. Centers for Disease Control and Prevention (CDC) started looking into an epidemic of unanticipated allergic-type responses in dialysis patients in early 2008, which started in 2007. The majority of them had received heparin intravenously from Baxter Healthcare. Additional analysis found that oversulfated chondroitin sulphate (OSCS), an artificial adulterant with hazardous effects, had been added during the production of heparin in China. Given its close resemblance to the original medication, routine testing was unable to identify OSCS, which is produced for roughly a hundred times less than heparin. (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012)A number of Americans experienced negative effects, including fatalities. At least 11 medication items and 72 healthcare products containing heparin were recalled by 14 additional American companies, including Baxter Healthcare, the main heparin producer in the United States. Heparin items were already suspended in Australia, Switzerland, Sweden, Denmark, Germany, France, and Italy as per regional health organisations and press sources. (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012)

The heparin scandal exposed a variety of supervision and supply chain management mistakes. Despite not doing a pre-approval examination, the FDA accepted SPL-CZ as a source for Baxter, in part because it mistook SPL-CZ for another website in its database. Investigators from Baxter were not allowed entry to upstream factories and aggregators in 2008 when they attempted to retroactively review their supply chain. (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012) Two heparin upstream consolidators were likewise off-limits to the FDA. Baxter started receiving heparin API produced by SPL-CZ in 2004, but somehow it didn't verify the facility until 2007; instead, it relied on an earlier evaluation by a separate business. A variety of production quality concerns were discovered during the investigation of SPL-CZ after the FDA discovered that it had been adulterated, including inadequate quality control procedures for incoming raw materials. SPL-CZ was not licensed by the Chinese State Food and Drug Administration since it was considered a chemical facility in China. It therefore probably received no supervision from the Chinese government. (Heparin: A Wake-Up Call on Risks to the U.S. Drug Supply, 2012)

Questions:

1. To avoid another situation like heparin adulteration in the future what steps should be taken by the government to protect people?
2. What could have been the major reason behind heparin adulteration? 
3. Do you think heparin contamination was intentional? Why or why not?

sources: 

1. Chinese Heparin Manufacturer again involved in Falsification and GMP Non-Compliance. (2016, march 2). Retrieved from gmp compilance:  [Accessed on: 2023 February 5]

Question- In the titration of a weak acid with a strong base, how would you calculate these quantities?

Multiple choice

Part A

initial pH

a. The initial pH is that of the strong base solution use for titration. Calculate the pH by working an equilibrium problem using the concentration of the weak acid as the initial concentration

Question 10 of 24

You make a Text Analytics API call.

You call the following URL.

You send the following body.

{

  "documents": [

    {

      "language": "en",

      "id": "1",

      "text": "Our tour guide took us up the Space Needle during our trip to Seattle last week."

    }

  ]

}

You receive the following response body

{

  "documents": [{

    "id": "1",

    "keyPhrases": ["Space Needle", "trip", "Seattle", "tour guide", "week"]

  }],

  "errors": []

}

The API identifies that the text was written a week after the tour.

Select Yes if the statement is true. Otherwise, select No.

Select only one answer.

1.  Yes

2.  No

The second equivalence point for the titration of a sodiumcarbonate unknown with 0.1001 M HCl is 35.10 mL. If the sample wasinitially dissolved in 50.00 mL of water, determine theconcentration of the carbonic acid, bicarbonate anion, hydroniumion, and hydroxide ions as well as the theoretical pH of thesolution when you have added only 20.55 mL of HCl. Given :Ka1= 4.44 x 10-7 and Ka2= 4.69 x 10-11

Formulas are below...

Concentration of CO3= [HCO3- ]+[H2CO3 ]
[H2CO3]= (total moles HCl added-molesHCl at first equivalence point)/total liters ofsolution
[HCO3-]=Concentration CO3 -[H2CO3]
[H+]=Ka1 [H2CO3 ]/ [HCO3-]

I just need someone else to do this so i can compare mynotes....Thanks

When creating a titration curve for a weak base, the pH of the initial solution requires setting up a table showing the initial, change, and equilibrium values for each species and plugging these into the equilibrium constant expression. The expression for the bicarbonate ion is Ka1=[H2CO3][H+][HCO3−] For an anion that can both hydrolyze and produce H+, the pH of a concentrated solution can be more easily approximated using the equation pH=12(pKa1+pKa2) During the titration before the equivalence point, provided that the concentration of acid is significantly more than the concentration of base, the Henderson-Hasselbalch equation can be used to approximate the pH: pH=pKa+log[base][acid] At the equivalence point, the solution is no longer a buffer, but contains the weak acid H2CO3. The change in concentration of the bicarbonate ion is significant, and the equilibrium constant expression for Ka1 must again be used to find the concentration of hydronium ions. After the equivalence point, the strong acid will control the pH.

Part A

A 10.0-mL sample of 1.0 M NaHCO3 is titrated with 1.0 M HCl (hydrochloric acid). Approximate the titration curve by plotting the following points: pH after 0 mL HCl added, pH after 1.0 mL HCl added, pH after 9.5 mL HCl added, pH after 10.0 mL HCl added (equivalence point), pH after 10.5 mL HCl added, and pH after 12.0 mL HCl added.

What is the antonyms of zigzag?

Part A

A 10.0-mL sample of 1.0 M NaHCO3 (sodium bicarbonate)is titrated with 1.0 M HCl(hydrochloric acid). Approximatethe titration curve by plotting the following points:

• pH after 0 mL HCl added,
• pH after 1.0 mL HCl added,
• pH after 9.5 mL HCl added,
• pH after 10.0 mL HCl added (equivalence point),
• pH after 10.5 mL HCl added, and
• pH after 12.0 mL HCl added.

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Part B

What volume of 0.170M HCl is required for the completeneutralization of 1.70g of NaHCO3(sodium bicarbonate)?

Express your answer to three significant figures and include theappropriate units.

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Part C

What volume of 0.200M HCl is required for the completeneutralization of 1.40g of Na2CO3(sodium carbonate)?

Express your answer to three significant figures and include theappropriate units.

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Part D

A sample of NaOH (sodium hydroxide) contains a small amount ofNa2CO3 (sodium carbonate). For titration to the phenolphthaleinendpoint, 0.120g of this sample requires 23.98 mL of 0.100MHCl. An additional 0.700 mL of 0.100 M HCl isrequired to reach the methyl orange endpoint. What is thepercentage of Na2CO3 by mass in the sample?

Express your answer to three significant figures and include theappropriate units.

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Match the concept vocabulary words to their definitions.

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.150 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

1. What volume of 0.200 M HCl is required for the complete neutralization of 1.20 g of Na2CO3 (sodium carbonate)?

2. A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.130 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

(I HAVE ONE ATTEMPT REMAINING PLEASE DO WELL)

Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43�10?7 and Ka2=4.73�10?11.

A) What volume of 0.200M HCl is required for the complete neutralization of 1.60g of NaHCO3(sodium bicarbonate)?

B)What volume of 0.170M HCl is required for the complete neutralization of 1.00g of Na2CO3(sodium carbonate)?

C) A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.180g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

What volume of 0.140M HCl is required for the complete neutralization of 1.40g of NaHCO3 (sodium bicarbonate)?

What volume of 0.200M HCl is required for the complete neutralization of 1.30g of Na2CO3 (sodium carbonate)?

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.150g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43�10?7 and Ka2=4.73�10?11. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation

NaHCO3(aq)+HCl(aq)?H2CO3(aq)+NaCl(aq)

1)What volume of 0.180M HCl is required for the complete neutralization of 1.50g of NaHCO3 (sodium bicarbonate)?

2)What volume of 0.120M HCl is required for the complete neutralization of 1.10g of Na2CO3 (sodium carbonate)?

3)A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.160g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110g of this sample requires 23.98 mL of 0.100 MHCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43�10?7 and Ka2=4.73�10?11. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation

NaHCO3(aq)+HCl(aq)?H2CO3(aq)+NaCl(aq)

Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110g of this sampleequires 23.98 mL of 0.100 MHCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?solutions are methyl orange and phenolphthalein.

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110g of this sample requires 23.98 mL of 0.100 MHCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43�10^-7 and Ka2=4.73�10^-11. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation

NaHCO3(aq)+HCl(aq)?H2CO3(aq)+NaCl(aq)

1)What volume of 0.180M HCl is required for the complete neutralization of 1.50g of NaHCO3 (sodium bicarbonate)?

2)What volume of 0.120M HCl is required for the complete neutralization of 1.10g of Na2CO3 (sodium carbonate)?

3)A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.160g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

Carbonic acid (H2CO3) is a weak diprotic acid with Ka1=4.43×10−7 and Ka2=4.73×10−11. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation

NaHCO3(aq)+HCl(aq)→H2CO3(aq)+NaCl(aq)

Part A

What volume of 0.190 M HCl is required for the complete neutralization of 1.70 g of NaHCO3 (sodium bicarbonate)?

Express your answer to three significant figures and include the appropriate units.

Part B

What volume of 0.120 M HCl is required for the complete neutralization of 1.80 g of Na2CO3 (sodium carbonate)?

Express your answer to three significant figures and include the appropriate units.

Part C

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.170 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

Express your answer to three significant figures and include the appropriate units.

A.Assuming you weighed out a 2.3684 g sample of your unknown, and dissolved and diluted it as in the procedure below, and it took 35.63 mL of a 0.1025 M HCl titrant to reach the endpoint, what are the weight percents of Na₂CO₃ and NaHCO₃ in your unknown sample? Solve the simultaneous equations similar to what we did in Ch 27.

Hints:

-Set g Na₂CO₃ = X

-Eqn A: bicarbonate + carbonate = diluted weighted mass (remember, the mass is not 2.3684, you diluted it before you titrated it. Calculate the diluted g of unknown)

-Convert the g of Na₂CO₃ to mol of HCl

-Convert the g of NaHCO₃ to mol of HCl

-mol HCl = mol HCl from Na₂CO₃ + mol HCl from NaHCO₃

-Before taking the final weight percent, undo the dilution to get back to the original wt % in the unknown

-Na₂CO₃ + 2HCl ↔ 2 NaCl + H₂O + CO₂

-NaHCO₃ + HCl ↔ NaCl + H₂O + CO₂

72.0 mL of a 1.60 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 155 mL of water. What is the final concentration? Assume the volumes are additive.

3) Convert 5.50 g of Na2CO3 to mol.

72.0 mL of a 1.80 M solution is diluted to a total volume of 228 mL. A 114-mL portion of that solution is diluted by adding 171 mL of water. What is the final concentration? Assume the volumes are additive.

72.0 mL of a 1.50 M solution is diluted to a total volume of 218mL. A 109-mL portion of that solution is diluted by adding 181 mLof water. What is the final concentration? Assume the volumes areadditive.

How can write python simple program

1. 72.0mL of a 1.50 M solution is diluted to a total volume of258 mL. A 129-mL poriton of that solution is diluted by adding 167mLof water. What is the final concentration? Assume the volumes areadditive? M=?

2.How many grmas of Na2CO3 are present in 21.0 mL. of a solutionthat is 31.0% Na2CO3 by mass. The density of hte solution is 1.12g/mL? g=?

How many grams of Na2CO3 are present in 15.5 mL of a solutionthat is 26.0% Na2CO3 by mass. The density of the solution is 1.14g/ml.

How many grams of Na2CO3 are present in 17.0 mL of a solutionthat is 39.0% Na2CO3 by mass. The density of the solution is 1.05g/mL.

How many grams of Na₂CO₃ arepresent in24.3 mL of a solution that is 26%Na₂CO₃ by mass. The density of the solutionis 1.17 g/mL

How many grams of Na2CO3 are present in 18.9 mL of a solution that is 32.0% Na2CO3 by mass. The density of the solution is 1.17 g/mL. ===? g

How many grams of Na2CO3 are present in 18.5 mL of a solution that is 20.0% Na2CO3 by mass? The density of the solution is 1.08 g/mL.