How many grams of NH.Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5. %3D PREV 1 2 3 NEXT > Based on your ICE table and definition of Ka, set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms. Ка %3D RESET [0] [1.00] [5.16] [1.8 x 10-1 [x] [2x] [0.5x] [6.9 x 10-] [0.709] [x + 6.9 x 10-] [x - 6.9 x 10-°] [x + 0.709] [x - 0.709] 1.8 x 10-5 4.7 5.6 x 10-10 1.8 x 10-19

How many grams of NH.Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5. %3D PREV 1 2 3 NEXT > Based on your ICE table and definition of Ka, set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms. Ка %3D RESET [0] [1.00] [5.16] [1.8 x 10-1 [x] [2x] [0.5x] [6.9 x 10-] [0.709] [x + 6.9 x 10-] [x - 6.9 x 10-°] [x + 0.709] [x - 0.709] 1.8 x 10-5 4.7 5.6 x 10-10 1.8 x 10-19

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

How many grams of NH.Br must be dissolved in 1.00L of water to produce a
solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5.
PREV
1
2
3
NEXT
Based on your ICE table and definition of Ka, set up the expression for Ka in order to determine
the unknown. Do not combine or simplify terms.
Ка
2 RESET
[0]
[1.00]
[5.16]
[1.8 x 10-1
[x]
[2x]
[0.5x]
[6.9 x 10-1
[0.709]
[x + 6.9 x 10-]
[x - 6.9 x 10-]
[x + 0.709]
[x - 0.709]
1.8 x 10-5
4.7
5.6 x 10-10
1.8 x 10-19

How many grams of NH.Br must be dissolved in 1.00 L of water to produce a
solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5.
2
3
NEXT
>
Let x represent the original concentration of NH:* in the water. Based on the given values, set up
the ICE table in order to determine the unknown.
NH. (aq)
H2O(1)
H:O*(aq)
NH:(aq)
+
+
Initial (M)
Change (M)
Equilibrium (M)
RESET
1.00
5.16
1.8 x 10-5
2х
0.5x
-2х
-0.5x
6.9 x 10-6
-6.9 x 10-6
0.709
-0.709
х+6.9 х 10 6
-x
x - 6.9 x 106
x + 0.709
x - 0.709

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Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 108. Complete Parts 1-4 before submitting your answer. 1 2 4 NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HCIO(aq) + OH(aq) 0.013 0.003 Before (mol) Change (mol) -0.013 0.013 After (mol) 0.010 0.003 H₂O(I) + CIO (aq) 0.037 0.003 0.040 RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040
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INTRODUCTION LABORATORY SIMULATION 1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH3COONa, in 78.0 mL of 0.10 Macetic acid, CH;COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5. pH E METHODS O RESET P MY NOTES A LAB DATA SHOW LABELS