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20 Nov 2019

The atomic weights of sodium, oxygen, and hydrogen are 23, 16, and 1, respectively. To neutralize 4 grams of NaOH dissolved in 1 L of water requires 1 L of:(A) 0.001 normal HCl solution(B) 0.01 normal HCl solution(C) 0.1 normal HCl solution(D) 1.0 normal HCl solutionPlease show step by step as to how to solve this problem. Thanks. Will Rate!!

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Sixta Kovacek
Sixta KovacekLv2
3 Sep 2019

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Related questions


1. Determine the amount of solute in the following samples:

500 ml of 0.2 M KI (potassium iodide)

220 ml of 0.03 M H2SO4 (sulfuric acid)

2.5 l of 0.1 M MgNO3 (magnesium nitrate)

1 ml of 5 M HCl (hydrochloric acid)

This problem requires that you know what molarity (M) is. M (molarity) = # of moles of solutes / Liter of solution. You are given the volume. You should be able to obtain moles of solutes. Your answers can be in moles or grams (either one will be acceptable).

2. How many ml of 0.1 M HCl would be required to titrate 35 ml of 1 M NaOH to the end point?

This is an acid/base reaction.

1) First, write out the balanced chemical reaction for HCl + NaOH.

2) Second, figure out the number of moles of NaOH in 35 ml of 1 M NaOH.

3) How many moles of HCl is required for completely reacting with the moles of NaOH in Part 2).

3. What is the pH of a 0.03 M solution of the strong base NaOH?

1) This question requires that you know pH = - log [H3O+], or simply as pH = - log [H+] (to make it easier).

2)So, you have to know how to use your scientific calculator to do log function (check Youtube).

3) This question also requires that you know: pOH = - log [OH-].

4) This question also requires that you know: [H3O+][OH-] = 1.0 x 10-14 or pH + pOH = 14

5) First step, determine the concentration of OH- in 0.03M NaOH when it dissociates or breaks up into Na+ and OH-.

6) This will give you [OH-]. You can plug this into pOH = - log [OH-] to get pOH.

7) Once you get pOH, then use (pH + pOH = 14) to get pH.

4. Balance the chemical reactions shown below and then write equilibrium expressions for each. All reactants and all products are in the gas phase.

CO + F2 ------> COF2

CH4 + O2 ------> CO2 + H2O

N2O4 -----> Br2 + NO

BrNO -----> Br2 + NO

1)This problem requires that you know how to balance chemical equations.

2)After you balance the equation, you need to know the equilibrium expression

5. Determine the oxidation states of each element comprising the following ionic compounds:

KClO4

NaMnO4

Sr(NO3)2

NaHCO3

CH4

Show all your steps for calculation questions in order to get full points.

1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).

2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.

a. Calculate the pH of the solution.

b. Calculate the concentrations of all species in this solution.

3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?

4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.

KOH, KCl, KCN, NH4Cl, HCl

5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.

6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?

H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7

7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:

a. before the titration starts.

b. after 8.00 mL of 0.100 M NaOH has been added.

c. at the half-way point of the titration.

d. at the equivalence point of the titration.

Show all your steps for calculation questions in order to get full points.

1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).

2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.

a. Calculate the pH of the solution.

b. Calculate the concentrations of all species in this solution.

3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?

4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.

KOH, KCl, KCN, NH4Cl, HCl

5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.

6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?

H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7

7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:

a. before the titration starts.

b. after 8.00 mL of 0.100 M NaOH has been added.

c. at the half-way point of the titration.

d. at the equivalence point of the titration.

e. after 52.00 mL of 0.100 M NaOH has been added.

8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25⁰C.

9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.

AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)

e. after 52.00 mL of 0.100 M NaOH has been added.

8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25⁰C.

9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.

AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)

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