Consider a buffer made from 255 mL 0.10 M HC2H3O2 and 125 mL 0.10 NaC2H3O2. Ka for HC2H3O2 is 1.8 x 10-5. Choose the true statement. A) Adding 25 mg NaOH (s) will reduce the pH. B) Adding 25 mL water will increase the pH. C) Adding 25 mL 0.0050 M HCI will increase the pH. D) Adding 25 mL 0.0050 M HF will reduce the pH. E) Adding 25 mg NaCl (s) will increase the pH.

Consider a buffer made from 255 mL 0.10 M HC2H3O2 and 125 mL 0.10 NaC2H3O2. Ka for HC2H3O2 is 1.8 x 10-5. Choose the true statement. A) Adding 25 mg NaOH (s) will reduce the pH. B) Adding 25 mL water will increase the pH. C) Adding 25 mL 0.0050 M HCI will increase the pH. D) Adding 25 mL 0.0050 M HF will reduce the pH. E) Adding 25 mg NaCl (s) will increase the pH.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH
Give a clear handwritten answer with explanation
1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL pure water.
Question 4 a) Determine the pH of 0.10 M NAOH solution. b) Find out the pH of a 0.002 M acetic acid solution if it is 2.3% ionised at this dilution. c) A chemistry student desires to prepare one litre of a solution buffered at pH 9.00. How many grams of ammonium chloride haye to be added to one litre of 0.20 M NH3 to makesuch a buffer. pKb value of ammonia is 4.75 in the equation. NH3 + H20 = NH + OH
0.05 mole of HCI is added to one liter of buffer containing 0.04 mole of NH,OH and 0.03 mole of NH,CI. What is the pH? (you can subtract add moles but not molarity)Kb = 1.8 X 10*
We have 500.0 mL of a buffer solution which is 0.651 M in NH3 and 0.354 M in NH4Cl. 500.0 mL of a 0.224 M HCl solution are added. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?
Consider the titration of 250.0 mL of 0.150 M HNO3 by 0.55 M NaOH. 1) Calculate the pH after 50.0 mL of NaOH has been added. 2) What volume of NaOH must be added so that the pH = 7.00?
3. A buffer solution contains 0.125 moles of ammonium chloride added to 500.0 ml of 0.500 M solution of ammonia. A) What is the pH of this buffer? B) What is the pH after the addition of 0.0100 moles of HCI bubbled into 500.0 mL of the buffer?
Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?
Calculate change in pH of a buffer solution
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74? Question 2 options: NH3 / NH4Cl (Ka = 5.6 × 10–10) NaNO2 / HNO2 (Ka = 4.5 × 10–4) CH3COONa / CH3COOH (Ka = 1.8 × 10–5) NaCl / HCl NaOCl / HOCl (Ka = 3.2 × 10–8)
4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.22 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH)