Question 1
Calculate the pH of a 0.020 mol L⁻¹ solution of potassium hydroxide (KOH) at 25 °C.
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Chemistry · Unit 3 · Chemical equilibrium systems · Chemical equilibrium
Calculate pH, hydrogen ion concentration [H+(aq)], pOH and hydroxide ion concentrations [OH–(aq)] for strong acids and bases. (Formula: pH = –log10 [H+] and pOH = –log10[OH–]) Brønsted-Lowry model
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Question 2
A 0.050 mol L$^{-1}$ solution of potassium hydroxide (KOH) is prepared at 25 °C. Calculate: (a) the hydroxide ion concentration [OH$^{-}$] in mol L$^{-1}$, (b) the pOH of the solution, (c) the pH of the solution. Show your working.
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Question 3
A solution of sodium hydroxide has a pOH of 2.40 at 298 K. What is the hydroxide ion concentration, [OH⁻], in this solution?
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Question 4
A solution of hydrochloric acid (HCl) has a concentration of $0.050 \text{ mol L}^{-1}$. Calculate the pH of this solution. Show your working.
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