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Sa We add some ammonium sulfate to water .What is the nature of the solution ,neutral,acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-10 and Kb (SO4) =8.3x10-¹13 Explain your reasoning. 86 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 M NaOH.After 40.00 mL of base was added the pH was 4.00. What is the Ka of the acid HA? 100 fodium acetate (MM-82.0,Kb-5.6x10-10)

Sa We add some ammonium sulfate to water .What is the nature of the solution ,neutral,acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-10 and Kb (SO4) =8.3x10-¹13 Explain your reasoning. 86 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 M NaOH.After 40.00 mL of base was added the pH was 4.00. What is the Ka of the acid HA? 100 fodium acetate (MM-82.0,Kb-5.6x10-10)

Chemistry
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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Please Show work for part 8a and explain your reasoning. As well as part 8b. Provide typed answer and concisely Thank you! Need asap
Sa We add some ammonium sulfate to water .What is the nature of the solution,neutral, acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-¹0 and Kb (SO4) =8.3x10-¹3 Explain your reasoning. 86 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 NaOH.After 40.00 mL of base was added the pH was 4.00.What is the Ka of the acid HA? int whon 0104 F sodium acetate (MM-82.0,Kb=5.6x10-¹0)
Transcribed Image Text:Sa We add some ammonium sulfate to water .What is the nature of the solution,neutral, acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-¹0 and Kb (SO4) =8.3x10-¹3 Explain your reasoning. 86 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 NaOH.After 40.00 mL of base was added the pH was 4.00.What is the Ka of the acid HA? int whon 0104 F sodium acetate (MM-82.0,Kb=5.6x10-¹0)
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