What is the difference between a strong acid and a weak acid? Give one example of each. What is meant by the ionic product for water, Kw? Define pH and hence calculate the pH of a solution of a) 0.01 M hydrochloric acid b) 0.1 M sodium hydroxide c) 0.2 M sulphuric acid d) 0.1 M butanoic acid, given that Ka = 1.51 x 10-5
Understanding the Concepts of pH and pOH, and the Relationships Surrounding Concentration, Moles, Molarity, and Number of Molecules
An aqueous solution of an unknown substance has a pH of 3.0. If you have 0.25 L of the substance, how many (a) H+ ions, and (b) OH-ions, are present?
Determine the pH of an aqueous solution prepared by mixing 50 mL of .125 M KOH with 50 mL of .125 M HCl while maintaining the temperature of the the system at 50 degrees C.
The pKa of HCN is 9.2. Calculate the Ka of HCN.
Amide ion (H<sub>2</sub>N-) is a stronger base than the hydroxide ion (OH-). Which would you expect to be a stronger acid, NH<sub>3</sub> or H<sub>2</sub>O? Why?
Picric acid (C<sub>6</sub>H<sub>3</sub>N<sub>3</sub>O<sub>7</sub>) has a pKa of 0.3. Formic acid (CHO<sub>2</sub>H) has a pKa of 3.7. Which is the stronger acid?
Ascorbic acid (vitamin C) has a pKa of 4.2 at 24 degrees Celsius. State the pH of the solution when the ratio of unprotonated to protonated forms of ascorbic acid is (a) 1:1 (b) 1:10 (c) 10:1 (d) 1:3 (e) Which form of ascorbic acid predominates at physiological pH?
Determining the pH of an acid and base in various situations by working with concentrations. A multi-step question.
Part 1: What is the pH of a solution of 1M HCO3 and 1M CO3? Part 2: What is the pH if it was mixed with an equal volume of water? Part 3: What is the pH if it was mixed with an equal volume of 0.001 M HCl? Part 4: What is the pH if it was mixed with an equal volume of 0.001 M NaOH?