Question
A 100 mL solution having 0.01 moles of NaOH dissolved in
it. The pH of the solution is:Solution
To find the pH of the solution, we first need to calculate the concentration of hydroxide ions ( OH-) in the solution, since NaOH dissociates completely in water to produce OH- ions. Given that the solution contains 0.01 moles of NaOH dissolved in 100 mL of solution, we can calculate the molarity (M) of NaOH: M= moles of solute/ volume of solution in liters So, M = 0.01 moles /0.1 L= 0.1 Π. Since NaOH dissociates completely, the concentration of OH ions is equal to the molarity of NaOH: [OH-] = 0.1 M Now, to find the pOH of the solution, we use the formula: POH = - log [OH-] POH = log(0.1) POH = -(-1) POH = 1 Finally, we can find the pH using the relation: pH + pOH = 14 pH = 14-pΠΠ pH = 14-1 pH = 13
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