Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to 1.000 L of the buffer solution. The new concentrationsare [HC,H3O2] = 0.4900 M and [C2H3O21] = 0.7100 M. The Ką = 1.60 x 10-5.everything is based upon the acid dissolving in water:HC2H3O2+ H20 <-> C2H3O21 + H3O*1[hKa[ isolve for [H3O+l] then put in the numbersKa [[H3O+'] =[[H3O*1] =pH = - log%3Df. SO3?a. H30+1b. Он1c. H2C6H6O6d. HCGH,061е. HSO31-2g. H2SO3h. HC2H3O2i. C,H3O21j. H2Sk. HS-1I. s2m. HXп. X1О. 1р. 2q. 3r. 0.5000s. 5.5 X 10-5t. 3.5 X 10-4u. 8.00 x 10-5v. 1.75 x 10-6w. 1.11 x 108х. 5.5 х 102у. О.7000z. 1.60 x 10-5аа. 1.143 х 10-5bb. 0.4900сс. 1.104 х 10-5dd. 0.7100ее. 1.26 х 10-5 ff. 4.901gg. 7.93hh. 4.942ii. 4.957

Here we are required to find the pH of the buffer solution after addition of 10 ml of 1M NaOH.

Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to 1.000 L of the buffer solution. The new concentrations are [HC2H302] = 0.4900 M and [C2H3O21] = 0.7100 M. The K, = 1.60 x 10-5. everything is based upon the acid dissolving in water: HC2H3O2 + H20 <-> C;H3O21 + H30+1 K = solve for [H30*1] then put in the numbers Ka [ [H3O*l] = [H3O*'] = pH = - log a. H30*1 b. Он1 c. H2C6H6O6 d. HCGH6O61 e. HSO31 f. SO3 2 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. S2 n. X-1 o. 1 р. 2 m. HX q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10:5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10:5 аа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957

Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to 1.000 L of the buffer solution. The new concentrations are [HC2H302] = 0.4900 M and [C2H3O21] = 0.7100 M. The K, = 1.60 x 10-5. everything is based upon the acid dissolving in water: HC2H3O2 + H20 <-> C;H3O21 + H30+1 K = solve for [H301] then put in the numbers Ka [ [H3Ol] = [H3O'] = pH = - log a. H301 b. Он1 c. H2C6H6O6 d. HCGH6O61 e. HSO31 f. SO3 2 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. S2 n. X-1 o. 1 р. 2 m. HX q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10:5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10:5 аа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957

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...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to 1.000 L of the buffer solution. The new concentrations
are [HC,H3O2] = 0.4900 M and [C2H3O21] = 0.7100 M. The Ką = 1.60 x 10-5.
everything is based upon the acid dissolving in water:
HC2H3O2
+ H20 <-> C2H3O21 + H3O*1
[h
Ka
[ i
solve for [H3O+l] then put in the numbers
Ka [
[H3O+'] =
[
[H3O*1] =
pH = - log
%3D
f. SO3?
a. H30+1
b. Он1
c. H2C6H6O6
d. HCGH,061
е. HSO31
-2
g. H2SO3
h. HC2H3O2
i. C,H3O21
j. H2S
k. HS-1
I. s2
m. HX
п. X1
О. 1
р. 2
q. 3
r. 0.5000
s. 5.5 X 10-5
t. 3.5 X 10-4
u. 8.00 x 10-5
v. 1.75 x 10-6
w. 1.11 x 108
х. 5.5 х 102
у. О.7000
z. 1.60 x 10-5
аа. 1.143 х 10-5
bb. 0.4900
сс. 1.104 х 10-5
dd. 0.7100
ее. 1.26 х 10-5 ff. 4.901
gg. 7.93
hh. 4.942
ii. 4.957

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