Homework Answers
The reaction is
a)
CH3COO- (aq) + H2PO4- (aq) <----------> CH3COOH (aq) + HPO4-2(aq)
BL base BL acid BL conjugate acid BL conjugate base
This is the net ionic equation.
b)The pKa of acetic acid is 4.74 and pKa of H2PO4- is 7.21 .
As the equilibrium always favors the side of weak acid- base pair, this equilibrium is shifted towards the reactants which are weak acid -base pair than the products.
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Use the References to access important values if needed for this question. (1) Write a net ionic equation for the reaction between H2SO3(aq) and HPO (aq) that shows H2SO3(aq) behaving as a Bronsted-Lowry acid. BL acid BL base BL base BL acid (2) Decide which would be favored at equilibrium for this reaction, reactants or products? products Submit Answer Retry Entire Group 2 more group attempts remaining
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[Review Topical References Use the References to access important values if needed for this question. Use the pull-down boxes to specify states such as (aq) or (8) If a box is not needed leave it blank. When aqueous solutions of potassium acetate and hydrobromic acid are mixed, an aqueous solution of potassium bromide and acetic acid results. Write the net ionic equation for the reaction. (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of...
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Use the References to access important values if needed for this question. Write a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant Knet for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s). Knet Submit Answer Retry Entire Group 8 more group attempts remaining Visited
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