17. Acid and Base Equilibrium
pH of Weak Bases
17. Acid and Base Equilibrium
pH of Weak Bases
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Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 × 10−10.
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An unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant.
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What is the pH of a 0.320 M solution of Ca(NO2)2 (ka of HNO2 is 4.5 × 10-4)?
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What is the pH of a 0.750 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?
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How can the pH of a solution be calculated if the pOH is known?
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The Kb of methylamine is 4.4 x 10–4. What is the approximate [OH–] of a 1 M solution of methylamine?
1101views - Scelta multipla15.3 grams of sodium benzoate is dissolved in 250 mL of water. What is the pH of the resultant solution if the Kb of benzoate ion is 1.5 x 10^-10?799views
- Scelta multiplaA 0.050 M solution of hydroxylamine, NH2OH, having Kb = 9.1 × 10^-9 has a pH of ________.1158views