Multiple Choice
If you have 500.0 mL of a 0.10 M solution of HClO, what mass of NaClO (molar mass = 74.44 g/mol) do you need to add to make a buffer with a pH of 7.5?
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18. Aqueous Equilibrium
Intro to Buffers
Multiple Choice
Which of the following represents the complete ionic equation for the reaction that occurs when a few drops of nitric acid (HNO3) are added to a buffer solution containing acetic acid (CH3COOH) and sodium acetate (CH3COONa)?
A
HNO3 + CH3COONa → CH3COOH + NaNO3
B
H+ + NO3- + CH3COO- + Na+ → CH3COOH + NO3- + Na+
C
HNO3 + CH3COOH → CH3COO- + H2O + NO3-
D
H+ + NO3- + CH3COOH → CH3COO- + H2O + NO3-
Verified step by step guidance1
Identify the species involved in the reaction. Nitric acid (HNO3) dissociates into hydrogen ions (H+) and nitrate ions (NO3-). Sodium acetate (CH3COONa) dissociates into acetate ions (CH3COO-) and sodium ions (Na+).
Write the complete ionic equation by representing all strong electrolytes as dissociated ions. For the given reaction, HNO3 dissociates into H+ and NO3-, and CH3COONa dissociates into CH3COO- and Na+.
Combine the dissociated ions from the reactants side: H+ + NO3- + CH3COO- + Na+.
Identify the products formed in the reaction. Acetic acid (CH3COOH) remains as a molecule, while sodium nitrate (NaNO3) dissociates into Na+ and NO3-.
Write the complete ionic equation for the products side: CH3COOH + NO3- + Na+. Ensure that the equation is balanced in terms of both mass and charge.
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