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

Please help out and show full solutions
A buffer is prepared by mixing 43.2 mL of 0.196 M NaOH with 141.2 mL of 0.231 M acetic acid. Calculate the pH of this buffer after the addition of 0.166 g of solid NaOH. (The pKa for acetic acid is 4.75.) (please type answer not write by hend)
ave to.) The K of acetic acid is 1.8 | 10. (Note: solid sodium acetate comes as a hydrate NaC2H3O2 3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer at pH 4.10, given that you will use 5.00 mL of 1.0 M acetic acid.
Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) (a no KOH added???? (b)20. mL of KOH solution added???? (c)39 mL of KOH solution added???? (d)40. mL of KOH solution added???? (e)41 mL of KOH solution added????
what volume of Boric acid 0.1 M and what volume of sodium hydroxide 0.1 M should be added together to produce a solution (buffer) with a pH of 9.1? (ka=6.0*10-10) 4H3BO3 +2NaOH --> Na2B4O7 +7H2O
3. What is the pH of a buffer produced by mixing 225 mL of 0.305 M HCOOH with 175 mL of 0.141 M KCOOH? Be sure to first find the new concentration of each compound in the mixed solution (M₁V₁ = M₂V₂ remember V₁ = total volume), then apply equilibrium.
How do I complete problem 1 in a step by step?
01 5 If the dissociation constant of a weak acid is 8.1 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order that has a pH of 4.09? prepare a buffer Oa) 0.100 M veak acid with 0.100 M conjugate base b) 0.100 M weak acid with 0.0100 M conjugate base Oc) 0.100 M weak acid with 0.0500 M conjugate base d) 1.000 M weak acid with 0.0100 M conjugate base e) 0.510 M weak acid with 0.0510 M conjugate base 0 000 О
Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate, NaC3H5O3 if 9.474 mL of 4.192 M NaOH is added. The total volume is 1.00 L. The Ka for lactic acid is 1.4*10-4.
Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If [HBrO] is 0.100 M, then what concentration of hypobromite ion is needed to achieve pH = 8.50
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
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