Be sure to answer all parts. The pH of a 0.064 M weak monoprotic acid is 3.09. Calculate the Ka of the acid. Ka =           ×10        Enter your answer in scientific notation.

A chemist dissolves 215. mg of pure potassium hydroxide in enough water to make up 90. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. x10

Consider the following data on some weak acids and weak bases: name acid hydrocyanic acid nitrous acid solution 0.1 M KCN 0.1 M HONH3Br 0.1 M NaNO2 0.1 M KBr formula HCN HNO2 Ka 4.9 × 10 4.5 x 10 X - 10 PH choose one ✓ Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one ✓ choose one choose one name S base formula hydroxylamine HONH₂ ethylamine C₂H5NH₂ | K₂ 1.1 × 10 6.4 × 10 8 4

A chemist dissolves 896. mg of pure sodium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. x10

A chemist dissolves 350. mg of pure sodium hydroxide in enough water to make up 100. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.

A chemist dissolves 465. mg of pure potassium hydroxide in enough water to make up 90. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.

1. A solution of 0.055 M propanoic acid, HC3H5O2, has a pH of (3.06x10^0). What is the Ka for propanoic acid? Express your answer to three significant figures. 2. Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonialike odor; it is used to remove hydrogen sulfide from natural gas. A 0.15 M aqueous solution of ethanolamine has a pH of (1.124x10^1). What is Kb for ethanolamine? Express your answer to three significant figures.

A solution has a hydroxide ion concentration of 3.5 × 10⁻⁹. Calculate the pH of the solution. Please give your answers to 2 decimal places.

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A chemist dissolves 423. mg of pure potassium hydroxide in enough water to make up 130. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.