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1) What is the pH of a 0.0235 M HCl solution? 2) What is the pOH of a 0.0235 M HCl solution? 3) What is the pH of a 6.50 x 10-3 M KOH solution? 4) A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-4 moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution?
In this set of practice problems, we will work on examples correlating the acidity and basicity of a solution with pH, calculating the pH of strong and weak acids and bases, the pH and pOH relationship, and calculating the pH of salt solutions.
We will calculate the pH of the solutions using the following 3 steps for each problem. Step 1: What is left in solution? Step 2: What are the equilibrium concentrations of the species in solution?
What is the pH of this solution? 1. What is the concentration of [H+] in a solution whose pH = 4.3? 2. What is the pH of a solution that has a Hydronium concentration of 3.4 x 10-‐3? 3. What is the pOH of a solution that has a pH of 6.8? 4. What is the concentration of Hydroxide . 7.
Find the pH of a 0.00476 M hydrochloric acid solution. 2. Write the equation for the dissociation of sulfuric acid. Find the pH of a solution that contains 3.25 g of H2SO4 dissolved in 2.75 liters of solution. 3. Write the equation for the dissociation of sodium hydroxide. Find the pH of a 0.000841 M solution of sodium hydroxide. 4.
30 lis 2018 · This downloadable PDF worksheet is for students to practice calculating pH and pOH values from concentration values of H + and OH-ions. Useful relationships: pH = -log[H + ] pOH = -log[OH - ] k water = 1 x 10 -14 = [H + ][OH - ] pH + pOH = 14
Directions: Solve the following pH calculations. Write the formula, plug numbers into formula, & give answer with correct units and significant figures. 1. If the pH of a solution is 10.3, what is the [H+] concentration? 2. If the [H+] is 2.1 × 10–12 M HClO4, what is the pH? Is the solution ACIDIC, BASIC, or NEUTRAL? 3.
