The pH of a basic solution is 10.65. What is [OH⁻]?

Classify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3

Sodium bicarbonate, NaHCO3, is used in baking powder formulations and in the manufacture of plastics and ceramics, among other things. If 26.3 g of the compound is dissolved in enough water to make 200. mL of solution, what is the concentration of NaHCO3? What are the concentrations of the ions in solution?

A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid must be neutralized (forming the potassium salt) for an important experiment. Calculate the volume of 0.221 M KOH that is needed to neutralize 24.93 g of the acid, forming K2A.

Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.

Hydroiodic acid often is used to disinfect and sanitize medical tools and products. In an experiment, 5.0 mL of 0.75 mol/L HI(aq) is mixed with 20.0 mL of distilled water. (record only your final answer with the correct number of significant digits and the proper units.) 1. What is the hydronium ion concentration of the resulting diluted solution? 2. What is the pH of the resulting solution?   3. If 1.0 mL of the diluted solution is added to 9.0 mL of distilled water, what is the resulting pH of the solution?   4. If 1.0 mL of the diluted solution from #3 is added to 9.0 mL of distilled water, you should be able to predict the pH based on the trend you see and without doing any calculations. This is because every time the hydronium concentration a) increases b)decreases by a factor of 10, the pH goes up one full unit since the solution becomes a)more b)less acidic.

The acidity of a solution is measured by its pH. If HT| represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 37.93% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 4.36, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number - (Report to the nearest 0.01)

The acidity of a solution is measured by its pH. If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 158 times greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 3.4, determine the pH of Solution A. Report your answer to one decimal place. Solution A has pH equal to Number (Report to the nearest 0.1)

It turns out that Ba(OH)2 is also considered a strong base. What is the [OH-] concentration in 0.34 M Ba(OH)2(aq) solution?

How many mL of 0.2 M HCl(aq) are needed to neutralize a 120 mL solution of 1.4 M Ba(OH)2?