2nd Edition

ISBN: 9780321809261

Author: John E. McMurry, Robert C. Fay

Publisher: Prentice Hall

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Textbook Question

Chapter 14, Problem 14.73SP

Calculate the pH of solutions prepared by:

(a) Dissolving 0.20 g of sodium oxide in water to give 100.0 mL of solution
(b) Dissolving 1.26 g of pure nitric acid in water to give 0.500 L of solution
(c) Diluting 40.0 mL of 0.075 M Ba(OH)₂ to a volume of 300.0 mL
(d) Mixing equal volumes of 0.20 M HCl and 0.50 M HNO₃ (Assume that volumes are additive.)

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Chapter 14, Problem 14.72SP

Chapter 14, Problem 14.74SP

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Can you please help mne with this problem. Im a visual person, so can you redraw it, potentislly color code and then as well explain it. I know im given CO2 use that to explain to me, as well as maybe give me a second example just to clarify even more with drawings (visuals) and explanations.

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Chapter 14 Solutions

General Chemistry: Atoms First

Ch. 14.1 - Write a balanced equation for the dissociation of...Ch. 14.1 - What is the conjugate acid of each of the...Ch. 14.1 - Prob. 14.3CP Ch. 14.1 - Some of the following ions have been detected...Ch. 14.2 - If you mix equal concentrations of reactants and...Ch. 14.2 - The following pictures represent aqueous solutions...Ch. 14.3 - Prob. 14.7P Ch. 14.4 - Prob. 14.8P Ch. 14.4 - The concentration of OH in a sample of seawater is...Ch. 14.4 - Prob. 14.10P

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Solution Summary: The author explains that pH is a logarithmic expression to express solutions are acidic, basic or neutral.

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