Calculate the pH of the solution resulting from the addition of 95 mL of 0.48 M HCl to 49 mL of 0.31 M aniline (C6H5NH₂). Kµ (C6H5NH₂) = 3.8 x 10-10

What is the pH of a saturated solution of Al(OH)3 at 25 oC, given that Ksp= 8.09 x 10-24 at this temperature?

Rainwater is slightly acidic due to dissolved CO₂. Use the following data to calculate the pH of unpolluted rainwater at 22.6°C: vol % in air of CO₂ = 0.063 vol%; solubility of CO2 in pure water at 22.6°C and 1.09 atm is 79.29 mL CO2 per 100 mL, K₁1 of H₂CO3 = 5.27x10-7. Express the pH with 2 decimals. You might have to solve a quadratic.

Suppose a 0.040M aqueous solution of oxalic acid (H2C2O4) is prepared. Calculate the equilibrium molarity of C2O4 2−. You'll find information on the properties of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits.

Calculate the molar concentration of OH− ions in a 0.077 M solution of ethylamine (C2H5NH2; Kb=6.4x10-4

When a 0.013 M aqueous solution of a certain acid is prepared, the acid is 0.73% dissociated. Calculate the acid dissociation constant K of the acid. Round your answer to 2 significant digits. x = 0 x10 X

Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 247 mL 0.0581 M 3‑(N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS is 7.18.

In the titration of 25.00 mL of a water sample, it took 20.590 mL of 3.150x 10−3 M EDTA solution to reach the endpoint.   The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)

What are the concentrations of H+ and OH− in asolution of 0.02 M NaOH?