Introduction to Chemistry
4th Edition
ISBN: 9781259288722
Author: BAUER
Publisher: MCG
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Chapter 13, Problem 110QP
(a)
Interpretation Introduction
Interpretation:
A balanced equation showing the acid and its conjugate base in equilibrium is to be written.
(b)
Interpretation Introduction
Interpretation:
The way in which the given buffer system prevents large
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What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml of 3.66M Sodium Formate (NaHCO2) together? If you were to now add 18 ml of 1.2M NaOH to the buffer solution, what would the new pH be?
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Chapter 13 Solutions
Introduction to Chemistry
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forward
- Write the equation for reaction of hydrofluoric acid and its conjugate base, fluoride ion with water. Show that the equations will give the auto ionisation equilibrium for water, and that Ka x Kb = Kw.arrow_forwardA)write expressions for pH and pOH of (NH4) 2SO4 B)write expressions for pH and pOH of NH4OHarrow_forwardDefine the term Buffer-Capacity?arrow_forward
- The ka of an unknown acid, HYO₂, is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1 M solution of HYO₂?arrow_forwardThe Ka of formic acid (HCO2H) is 1.8x10-4. What would the pH of a solution containing equal concentrations of formic acid and sodium formate be? Use the H-H equation for buffers to solve this. This is true in general for solutions where the acid and conjugate base are present in equal concentrations.arrow_forwardWrite the Ka (acid ionization equilibrium constant) expression for the ionization of HC3H5O2 in water.arrow_forward
- A 250.0 mL sample of 0.4375 M aniline, C6H5NH2 (Kb = 3.8 x 10-10) reacted with 2.250 L of gaseous hydrocyanic acid, HCN (Ka = 6.2 x 10-10) at 25.0°C and 8353.0 mmHg. Assuming the volume of the solution did not change, calculate the pH and concentrations of all species present at equilibrium.arrow_forwardCalculate the ph of a solution prepared by dissolving 1.75g of sodium acetate, CH3COONa, in 78.0 mL of 0.15 M acetic acid, CH3COOH (aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75x10^-5arrow_forwardWhat is the pH of a sodium acetate (NaCH3CO2) solution prepared by adding 0.820 g of sodium acetate to 100.0 mL of water at 25 ℃? The Ka of acetic acid at 25 ℃ is 1.8 x 10–5.arrow_forward
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