A solution is prepared at 25 °C that is initially 0.36M in diethylamine ((C₂H₂)₂NH), bromide ((C₂H₂)NH₂Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X NH, a weak base with K = 1.3 x 10 and 0.18M in diethylammonium

A solution is prepared that is initially 0.38M in ethylamine (C₂H5NH₂), a weak base, and 0.12M in ethylammonium chloride (C₂H5NH₂C1). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH-]. You can leave out the M symbol for molarity. initial change final [C,HẠNH,] 0 0 [C,HẠNH] 0 0 [OH-] 0 010 X Ś

A solution is prepared at 25 °C that is initially 0.48 M in diethylamine ((C,H5)¸NH), a weak base with K,=1.3 × 10 -3 and 0.024M in diethylammonium bromide ((C,H5) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH olo Ar

A chemist must prepare 450.0 mL of nitric acid solution with a pH of 1.60 at 25 °C. He will do this in three steps: • Fill a 450.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (5.0M) 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 400.0 mL of hydrochloric acid solution with a pH of 1.20 at 25 °C. He will do this in three steps: • Fill a 400.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (8.0M) stock hydrochloric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. |mL x10

161P.) The ionization constant of a very weak acid, HA, is 1.5×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] =  mol/L [A-] =  mol/L [HA] =  mol/L pH =

A chemist dissolves 891. mg of pure hydrochloric acid in enough water to make up 270. mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. ☐ ☐ x10

Phosphoric acid, H₂PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.500 M phosphoric acid solution. [H₂PO₂] = [H₂PO] = [HPO²] = [PO³] = M M M M pKal 2.16 [H+] = [OH-] = pH = pK₂2 7.21 pK₂3 12.32 M M

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A solution is made by dissolving 5.315 g of hydrocyanic acid (HCN, 27.062 g/mol, K- 6.17 x 10-10) and 7397 g of potassium cyanide %3D (KCN, 65.116 g/mol) in enough water to make 750.0 mL of solution. Calculate the pH of this solution after 19.74 mL of a 1L814 M NAOH solution has been added to it.