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Does the pH of the solution increase, decrease, or stay the same when you (a) add solid sodium oxalate, Na 2 C 2 O 4 , to 50.0 mL of 0.015 M oxalic acid, H 2 C 2 O 4 ? (b) add solid ammonium chloride to 75 mL of 0.016 M HCl? (c) add 20.0 g of NaCl to 1.0 L of 0.10 M sodium acetate, NaCH 3 CO 2 ?

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17, Problem 2PS
Textbook Problem
313 views

Does the pH of the solution increase, decrease, or stay the same when you

  1. (a) add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015 M oxalic acid, H2C2O4?
  2. (b) add solid ammonium chloride to 75 mL of 0.016 M HCl?
  3. (c) add 20.0 g of NaCl to 1.0 L of 0.10 M sodium acetate, NaCH3CO2?

a)

Interpretation Introduction

Interpretation:

pH of the solution will increase, decrease or remains same has to be predicted.

Concept introduction:

pH of a solution is basically the measure of the molar concentration of the H+ ion in the solution. More the concentration of H+ ion in the solution, lower will be the pH value and more acidic will be the solution.

The expression for pH is given as,

pH=log[H+]

 pOH of a solution is basically the measure of the molar concentration of the OH ion in the solution. More the concentration of OH ion in the solution lower will be the value of pOH and more basic will be the solution.

The expression for pOH is given as,

pOH=log[OH]

pH is calculated using following relation.

pH+pOH=14

Common ion effect is defined as the phenomenon of the suppression of the dissociation of weak acid or base in presence of strong electrolyte having a common ion.  The common ion effect changes pH of the solution.

For example, a weak acid HA undergo partial dissociation in aqueous solution and an equilibrium is established between the dissociated and undissociated acid given as follows,

  HA(aq.)+ H2O(l)H3O+(aq.)+ A1(aq.)

Now if in the solution strong electrolyte having a common ion H3O+ or  A1 is added then according to the Le-Chatelier’s principle if the concentration of any of the product will increase then the reaction equilibrium will move to that side of the equilibrium that will decrease the effect of increased concentration of the product. Therefore the reaction will move in a backward direction forming more of undissociated acid and decrease the concentration of H3O+ in the solution, as a result, pH of the solution will increase.

Explanation of Solution

An aqueous solution oxalic acid is a weak base  and dissociates as follows,

  H2C2O4(aq)2H+(aq)+C2O42(aq)

If solid sodium oxalate Na2C2O4 is added to the solution then the concentration of H+ ions will decrease as Na2C2O4 is a strong electrolyte and will dissociate in aqueous solution giving Na+ and C2O42 ions

(b)

Interpretation Introduction

Interpretation:

pH of the solution will increase, decrease or remains same has to be predicted.

Concept introduction:

pH of a solution is basically the measure of the molar concentration of the H+ ion in the solution. More the concentration of H+ ion in the solution, lower will be the pH value and more acidic will be the solution.

The expression for pH is given as,

pH=log[H+]

 pOH of a solution is basically the measure of the molar concentration of the OH ion in the solution. More the concentration of OH ion in the solution lower will be the value of pOH and more basic will be the solution.

The expression for pOH is given as,

pOH=log[OH]

pH is calculated using following relation.

pH+pOH=14

Common ion effect is defined as the phenomenon of the suppression of the dissociation of weak acid or base in presence of strong electrolyte having a common ion.  The common ion effect changes pH of the solution.

For example, a weak acid HA undergo partial dissociation in aqueous solution and an equilibrium is established between the dissociated and undissociated acid given as follows,

  HA(aq.)+ H2O(l)H3O+(aq.)+ A1(aq.)

Now if in the solution strong electrolyte having a common ion H3O+ or  A1 is added then according to the Le-Chatelier’s principle if the concentration of any of the product will increase then the reaction equilibrium will move to that side of the equilibrium that will decrease the effect of increased concentration of the product. Therefore the reaction will move in a backward direction forming more of undissociated acid and decrease the concentration of H3O+ in the solution, as a result, pH of the solution will increase.

(c)

Interpretation Introduction

Interpretation:

pH of the solution will increase, decrease or remains same has to be predicted.

Concept introduction:

pH of a solution is basically the measure of the molar concentration of the H+ ion in the solution. More the concentration of H+ ion in the solution, lower will be the pH value and more acidic will be the solution.

The expression for pH is given as,

pH=log[H+]

 pOH of a solution is basically the measure of the molar concentration of the OH ion in the solution. More the concentration of OH ion in the solution lower will be the value of pOH and more basic will be the solution.

The expression for pOH is given as,

pOH=log[OH]

pH is calculated using following relation.

pH+pOH=14

Common ion effect is defined as the phenomenon of the suppression of the dissociation of weak acid or base in presence of strong electrolyte having a common ion.  The common ion effect changes pH of the solution.

For example, a weak acid HA undergo partial dissociation in aqueous solution and an equilibrium is established between the dissociated and undissociated acid given as follows,

  HA(aq.)+ H2O(l)H3O+(aq.)+ A1(aq.)

Now if in the solution strong electrolyte having a common ion H3O+ or  A1 is added then according to the Le-Chatelier’s principle if the concentration of any of the product will increase then the reaction equilibrium will move to that side of the equilibrium that will decrease the effect of increased concentration of the product. Therefore the reaction will move in a backward direction forming more of undissociated acid and decrease the concentration of H3O+ in the solution, as a result, pH of the solution will increase.

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Chapter 17 Solutions

Chemistry & Chemical Reactivity
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Ch. 17.3 - The titration of 0.100 M acetic acid with 0.100 M...Ch. 17.3 - Calculate the pH after 75.0 mL of 0.100 M HO has...Ch. 17.3 - 1. What is the pH after 25.0 ml of 0.100 M NaOH...Ch. 17.3 - 2. What is the pH at the equivalence point in the...Ch. 17.3 - Use Figure 17.10 to decide which indicator is best...Ch. 17.3 - Phosphate ions are abundant in cells, both as the...Ch. 17.3 - A typical total phosphate concentration in a cell,...Ch. 17.4 - The barium ion concentration, [Ba2+], in a...Ch. 17.4 - Calculate the solubility of AgCN in moles per...Ch. 17.4 - Calculate the solubility of Ca(OH)2 in moles per...Ch. 17.4 - Calculate the solubility of BaSO4 (a) in pure...Ch. 17.4 - 12. Calculate the solubility of Zn(CN)2 at 25°C...Ch. 17.4 - What is the Ksp expression for silver carbonate?...Ch. 17.4 - 2. Using Ksp values, predict which salt in each...Ch. 17.4 - What is the solubility of PbSO4 in water at 25C?...Ch. 17.4 - 4. What is the solubility of PbSO4 in water at...Ch. 17.4 - Which compound should be more soluble in 0.1 MHCl...Ch. 17.5 - Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker...Ch. 17.5 - What is the minimum concentration of I that can...Ch. 17.5 - You have 100.0 mL of 0.0010 M silver nitrate. Will...Ch. 17.5 - 1. Will SrSO4 precipitate from a solution...Ch. 17.6 - Silver nitrate (0.0050 mol) is added to 1.00 L of...Ch. 17.6 - 1. Iron(II) chloride (0.025 mol) is added to 1.00...Ch. 17.7 - Calculate the value of the equilibrium constant,...Ch. 17.7 - 1. What is the equilibrium constant for the...Ch. 17.7 - Approximately 0.10 g of sodium cyanide is fatal to...Ch. 17.7 - What is the minimum volume of 0.0071 M NaCN(aq)...Ch. 17.7 - Use the formation constant of [Au(CN)2] in...Ch. 17.7 - Silver undergoes similar reactions as those shown...Ch. 17.7 - Write a balanced chemical equation for the...Ch. 17 - Does the pH of the solution increase, decrease or...Ch. 17 - Does the pH of the solution increase, decrease, or...Ch. 17 - What is the pH of a solution that consists of 0.20...Ch. 17 - What is the pH of 0.15 M acetic acid to which 1.56...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the buffer solution that...Ch. 17 - Lactic acid (CH3CHOHCO2H) is found in sour milk,...Ch. 17 - What mass of sodium acetate, NaCH3CO2, must he...Ch. 17 - What mass of ammonium chloride, NH4Cl, must be...Ch. 17 - Calculate the pH of a solution that has an acetic...Ch. 17 - Calculate the pH of a solution that has an...Ch. 17 - What must the ratio of acetic acid to acetate ion...Ch. 17 - What must the ratio of H2PO4 to HPO42 be to have a...Ch. 17 - A buffer is composed of formic acid and its...Ch. 17 - A buffer solution is composed of 1.360 g of KH2PO4...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Describe how to prepare a buffer solution from...Ch. 17 - Describe how to prepare a buffer solution from NH3...Ch. 17 - Determine the volume (in mL) of 1.00 M NaOH that...Ch. 17 - Determine the volume (in mL) of 1.00 M HC1 that...Ch. 17 - A buffer solution was prepared by adding 4.95 g of...Ch. 17 - You dissolve 0.425 g of NaOH in 2.00 L of a buffer...Ch. 17 - A buffer solution is prepared by adding 0.125 mol...Ch. 17 - What is the pH change when 20.0 mL of 0.100 M NaOH...Ch. 17 - Phenol, C6H5OH, is a weak organic acid. 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