A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any HNO3. The Kp of NH3 is 1.8 x 10-5.

Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10–5. What is the pH after 15.00 mL of HCl have been added?

100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 30.0 mL 0.10 M HNO3. The K₁ of NH3 is 1.8 × 10-5. 4.38 9.62 8.56 5.44

Calculate the pH of a buffer that is 0.12M lactic acid and 0.10M sodium lactate. The Ka for lactic acid is 1.4 x 10-4.

5 mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5 What is the pH of the solution at the equivalence point? What is the pH of the solution after the addition of 10ml of HCl?

o A 55.0 mL solution of 0.150 M potassium alaninate ( H₂NC₂H₂CO₂K) is titrated with 0.150 M HCl. The pKa values for the amino acid alanine are 2.344 (pKal) and 9.868 (pK₂2), which correspond to the carboxylic acid and amino groups, respectively. Calculate the pH at the first equivalence point. pH = Calculate the pH at the second equivalence point. pH = H₂N- CH3 -CH- K Potassium Alaninate

A buffer at pH 5.1 is prepared from a total concentration of 0.278 M sodium acetate and acetic acid. What are the concentrations of acetic acid and acetate in this solution? The Ka for acetic acid is 1.76 x 10-5 and the pKa is 4.75.

A 75.0 mL sample of 0.100M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the resulting solution after the addition of 100.0 mL of HCl to the NH3? Kp, NH3 = 1.8x10-5 O the pH would be exactly 1 O the pH is = 7.545 O the pH = 5.277 O pH = 1.845

A 25.0 mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.

A friend tells you: " The constant K sp of a salt is called the sol ubility product constant and is calculated from the concentra tions of ions in the solution . Thus, if salt A dissolves to a greater extent than salt B , salt A must have a higher K sp than salt B. Do you agree with your friend ? Explain . Explain the following phenomenon You a test tube with