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Write the balanced total ionic equation and the net ionic equation (including phase labels) for the reaction between HCl(aq) and NaOH(aq). Toatal Ionic: Net Ionic: Assume that you took 39.0 mL of 0.050 M HCl(aq) and 39.0 mL of 0.050 M NaOH(aq) and mixed them together to perform the reaction. List the ions that remain after the reaction finished. (Choose all that apply) H^+(aq) OH^-(aq) Cl^-(aq) Na^+(aq) H_3O^+(aq) H_2)(l) Calculate the molar concentration of each ion. Remember that a dilution occurred when the HCl(aq) and the NaOH(aq) solutions were combined. Notice: In this case, it doesn't matter which ions remain, they would all have the same concentration, so you need only enter in one answer regardless of what you chose in the multiple choice question.
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Related questions
The following data were collected at 20 oC for the reaction of bromophenol blue (HBPB2-) and hydroxide ions (OH-):
HBPB2- (aq) + OH- (aq) ---> BPB3- (aq) + H2O (l)
The times required to form a constant [BPB3-] at varying initial concentrations of reactants were determined and tabulated. From the rate data, determine the rate law for the reaction.
trial | [OH-] | [HBPB2-] | reaction time (sec) | rate (1/sec) |
1 | 1.00 | 7.22 x 10-6 | 75 | |
2 | 0.25 | 7.22 x 10-6 | 290 | |
3 | 1.00 | 3.63 x 10-6 | 152 |
rate = k[HBPB2-]2[OH-] | ||
rate = k[HBPB2-]2[OH-]2 | ||
rate = k[HBPB2-][OH-] | ||
rate = k[HBPB2-][OH-]2 |
QUESTION 2
Which of the following balanced molecular equations represent reactions for which the rate law expression could likely be determined via time to turbidity determinations? Select all that apply.
a. | 2 KI (aq) + Pb(NO3)2 (aq) ---> PbI2 (s) + 2 KNO3 (aq) | |
b. | 2 HBr (aq) + Ca(OH)2 (aq) ---> 2 H2O (l) + CaBr2 (aq) | |
c. | 2 NO (g) + 5 H2 (g) ---> 2 NH3 (g) + 2 H2O (g) | |
d. | FeS (s) + HCl (aq) ---> FeCl2 (aq) + H2S (g) | |
e. | 3 SrCl2 (aq) + 2 Li3PO4 (aq) ---> Sr3(PO4)2 (s) + 6 LiCl (aq) |
QUESTION 3
When working in the laboratory a small amount of 0.30 M sodium thiosulfate accidentally splashes on your exposed forearm. What should you do? Select all that apply.
a. | Inform your lab instructor. | |
b. | Proceed immediately to the sink in the laboratory and flush the area with copious amounts of water. Then wash the area with mild hand soap. | |
c. | Leave the laboratory immediately. All lab work is over for you today. | |
d. | Do nothing. | |
e. | Stop, drop, and roll. |
QUESTION 4
volume of 1.0 M HCl | volume of water | volume of 0.3 M Na2S2O3 | |
well 1 | 2.0 mL | 0 | 3.0 mL |
well 2 | 2.0 mL | 1.5 mL | 1.5 mL |
well 3 | 2.0 mL | 2.0 mL | 1.0 mL |
The above table summarizes the amounts and concentrations of the reactants that will be used in each trial in Parts II. Use the dilution equation, M1V1 = M2V2, to calculate the concentration Mf (molarityfinal) of Na2S2O3 in each well after mixing but before any reaction occurs. The [HCl] has been worked for you as an example.
M1(HCl)V1 = M2(HCl)V2 where V2 = final total volume Vf
(1.0 M)(2.0 mL) = M2(HCl)(5.0 mL)
M2(HCl) = 0.40 M = Mf(HCl)
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