A 25.0-mL sample of 0.150 M hydrocyanic acid, HCN, is titrated with a 0.150 M NaOH...

A 25.0-mL sample of 0.150 M hydrocyanic acid, HCN, is titrated with a 0.150 M NaOH solution. What is the pH after 16.3 mL of base is added? The K a of hydrocyanic acid is 4.9 × 10 -10.

A 25.0 mL sample of 0.150 M hydrocyanic acid, HCN, is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K a of hydrocyanic acid is 4.9 × 10 -10.

What is the pH of a 0.100 M NH 3 solution that has K b = 1.8 × 10 -5 ?

If a 5.00 g sample of an unknown nonelectrolyte was dissolved in 50.00 g of water, whose K_f =1.86 °C/m, and the resulting freezing point was -3.00 °C. What is the molar mass of the unknown nonelectrolyte solute.

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queen_honey_blossom answered 1 year ago

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