Use the scenario to answer the following question. A group of students working in a chemistry lab is planning a procedure to neutralize 25.0mL of 2.0 M hydrochloric acid (strong acid) with 1.0 M potassium hydroxide (strong base). In their procedure they plan on adding an equal volume of the base to the acid. What would be the expected outcome of carrying out this step as planned? O A. The resulting pH will be equal to 7 because a strong base will neutralize a strong acid. B. The resulting pH will be greater than 7 because potassium hydroxide is less concentrated than the hydrochloric acid. C. The resulting pH will not be able to be determined because the concentrations of the acid and base are not the same. D. The resulting pH will be less than 7 because potassium hydroxide is less concentrated than the hydrochloric acid.

Finding pH An unknown substance has a hydrogen ion concentration of 3H 4  3.1  108M. Find the pH and classify the substance as acidic or basic

A student is provided with a stock solution of NaOH with 0.1 M concentration. A 25.0 mL of stock solution of NaOH is diluted with water to prepare 500.0 mL NaOH a.Calculate the molarity of the final diluted  b.Calculate the hydronium ion concentration, [H3O+] in the final  c.Calculate the pH of the diluted NaOH solution  d.Is the final diluted solution acidic, basic or neutral?

A chemist must prepare 600.0 mL of sodium hydroxide solution with a pH of 13.40 at 25 °C. She will do this in three steps: • Fill a 600.0 mL volumetric flask about halfway with distilled water. Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. x10 ?

A chemist dissolves 890. mg of pure barium hydroxide in enough water to make up 110. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. x10

A chemist must prepare 850.0 mL of sodium hydroxide solution with a pH of 12.60 at 25 °C. He will do this in three steps: • Fill a 850.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. Ox10

Consider the following data on some weak acids and weak bases: name acetic acid hydrocyanic acid acid solution 0.1 M KCH3CO₂ 0.1 M NaBr 0.1 M NaCN 0.1 M C5H5NHCI Ka formula HCH3CO2 1.8 × 10 HCN 4.9 × 10 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. X pH - 10 -5 choose one choose one ✓ choose one choose one Ś base K₂ formula C6H5NH₂ 4.3 × 10 -10 -9 1.7×10 ⁹ name aniline pyridine CH-N

A chemist must prepare 900.0 mL of sodium hydroxide solution with a pH of 13.40 at 25 °C. He will do this in three steps: • Fill a 900.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. Ox10

A chemist dissolves 522. mg of pure potassium 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.) Round your answer to 3 significant decimal places. x10 5

A stock solution of hydrochloric acid has a concentration of 0.1200M. It is diluted by transferring 10.00 mL to a 100mL volumetric flask using a volumetric pipette. Based on calculations it is found the pH is 1.92. Using the solution that was diluted, prepare a solution with a pH of 2.912. What volume of the diluted solution should you dilute to 100.00 mL to make this solution?