Arrange the following 0.1 M aqueous solutions in order of increasing pH:  NaOH, HBr, NaCH3CO2, KBr, NH4Br

Predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name formula hydrocyanic acid HCN hydrofluoric acid HF acid solution 0.1M NaCN 0.1MKCI 0.1MKF 0.1MHONH, CI K₁ 4.9 × 10 10 6.8 x 10 PH -4 base 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. K₂ formula hydroxylamine HONH₂ 1.1 x 10 0-8 pyridine C₂H₂N 1.7 x 109 name

A chemist must prepare 700.0 mL of sodium hydroxide solution with a pH of 12.30 at 25 °C. She will do this in three steps: • Fill a 700.0 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

For the diprotic weak acid H2A, ?a1 = 2.3×10−6 and ?a2  = 6.8×10−9. What is the pH of a 0.0500 M solution of H2A? pH=     What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]=                                                       M     [A2−]=                                                        M

Determine the pH of each of the following solutions. 0.19 M CH3NH3I(Kb(CH3NH2)=4.4×10^−4) Express your answer to two decimal places.

A chemist must prepare 650.0 mL of nitric acid solution with a pH of 1.70 at 25 °C. He will do this in three steps: • Fill a 650.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (9.0M) stock nitric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated nitric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. mL x10 ?

A chemist must prepare 800.0 mL of potassium hydroxide solution with a pH of 12.80 at 25 °C. She will do this in three steps: • Fill a 800.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid potassium hydroxide and add it to the flask. Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. ☐ g ☐ x10

Calculate the pH of a solution that has a hydronium ion concentration, [H3O+],[H3O+], of 5.79×10−5 M.

pH is a logarithmic scale used to indicate the hydrogen lon concentration, [H], of a solution: pH = -log[H] Due to the autoionization of water, in any aqueous solution the hydrogen lon concentration and the hydroxide ion concentration, (OH], are related to each other by the K of water K.-HOH -1.00 x 10-¹4 where 1.00 x 104 is the value at approximately 297 K Based on this relation, the pH and pOH are also related to each other as 14.00 pH + POH The temperature for each solution is camned out at approximately 297 K Part A ▸ 0.55 g of hydrogen chloride (HCT) is dissolved in water to make 55L of solution. What is the pll of the resulting hydrochionc acid solution? Express the pH numerically to two decimal places. View Available Hint(s) 10 ΑΣΦ pH-2.42 Submit Previous Answer X Incorrect; Try Again; 2 attempts remaining Part B pH- K.-1.00×10 0.55 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 5.5 L of soution What is the pill of thon? Express the pH numerically to two…

At 25 °C, what is the hydroxide ion concentration, [OH−], in an aqueous solution with a hydrogen ion concentration of [H+]=4.8×10^−7M?