Interpretation:
To calculate the
Concept introduction:
Answer to Problem 43QAP
Explanation of Solution
At
For above reaction equilibrium constant K is:
Given,
The value of equilibrium constant
Hence,
Thus,
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Chapter 21 Solutions
Chemistry: Principles and Reactions
- Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) _________ (aq) + Br(aq) NH3(aq) + HBr(aq) (b) CH3COOH(aq) + CN(aq) ________ (aq) + HCN(aq) (c) ________ (aq)+H2O () NH3(aq) + OH(aq)arrow_forwardThe hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.arrow_forwardWhen carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)arrow_forward
- What is the pH of a 1.00 molar solution of NH4Cl(aq)? The Kb for NH3 = 1.8 × 10–5 .arrow_forwardThe pH of an aqueous solution of 8.39×10-2 M ammonium nitrate, NH4NO3 (aq), isarrow_forward8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?arrow_forward
- What is the pH of a 1.00 molar solution of NaCN(aq)? The Ka for HCN = 6.2 × 10–10 .arrow_forwardCalculate the equilibrium concentrations of all chemical species present in a 0.10 M H2CO3(aq) solution. What is the percent ionization of the acid and resulting pH?arrow_forwardHA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C.arrow_forward
- Calculate the pH at 25 °C of a solution that is 1.00 M in NaClO(aq) and 2.00 M in HClO(aq). For HClO, Ka = 6.8×10−4 at 25 °C.arrow_forwardWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution.ClO- (aq) + H2O (l)HClO (aq) + OH- (aq)arrow_forwardThe pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) isarrow_forward
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