Chapter 7: Q7-117E (page 240)
Question: Determine the pH of a 0.50 M solution of NH4OCl.
Answer
pH of the given solution comes out to be 8.4.
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Consider the following illustrations:
Which beaker best illustrates what happens when the following acids are dissolved in water?
a. HNO2 b. HNO3 c. HCl d. HF e. HC2H3O2
Question:Can the pH of a solution be negative? Explain. True or false: A strong acid solution always has a lower pH than a weak acid solution. Explain.
An acid HX is 25% dissociated in water. If the equilibrium concentration of HX is 0.30 M, calculate the Ka value for HX.
Question: Calculate the pH and [S2-] in a 0.10 M H2S solution. Assume Ka1 = 1.0 × 10-7; Ka2 = 1.0 × 10-19.
Use Table 7.3 to help answer the following questions.
a. Which is the stronger acid, HClO4 or C6H5NH3+?
b. Which is the stronger acid, H2O or C6H5NH3+?
c. Which is the stronger acid, C6H5NH3+or CH3NH3+?
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