Question 29: Calculate the pH of the following aqueous salt solutions. Report your calculated pH to 2 decimal places. 0.100 M NaCl: 0.032 M NH4Br: 0.093 M KNO2:

A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume of water must be added to change the pH to 4.000?

Follow the instructions of Question 7 for the hydrogen carbonate ion, HCO3-.

Which of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH] > 1.0 X IO’7M

Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2

The nickel(II) ion exists as [Ni(H2O)4]2+ in aqueous solution. Why is this solution acidic? As part of your answer, include a balanced equation depicting what happens when [Ni(H2O)6]2+ interacts with water.

A sample of coffee has a pH of 4.3. Calculate the hydronium ion concentration in this coffee. Is the coffee acidic or basic?

Classify the solutions represented in Exercises 9.27 and 9.29 as acidic, basic, or neutral.

. For a hydrogen ion concentration of 2.33106M, how many decimal places should we give when expressing the pH of the solution?

What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?