Find the pH of a 0.205 M HClO2(aq) solution. For H...

Question

Find the pH of a 0.205 M HClO2(aq) solution. For HClO2, Ka =0.011.

Jules Bruno · Accepted Answer

We’re being asked to calculate the pH of a 0.205 M HClO2HC3H5O2 is a weak acid that will further react in water to form H3O+HClO2 (aq) + H2O (l) → H3O+ (aq) + ClO2- (aq)We can use the H3O+ produced to find the pH[readmore]From this, we can construct an ICE table for the reaction of HlClO2 in a solution. Remember that liquids are ignored in the ICE table.The Ka expression for HClO2(aq) isWe can now plug in the equilibrium concentrations and solve for xKa=[products][reactants]=[H3O+][ClO2-][HClO2]When writing equilibrium expressions:• Solids and liquids are not included in the expressionWe can now plug in the equilibrium concentrations and solve for xKa=[products][reactants]=[H3O+][ClO2-][HClO2]Ka=0.011=(x)(x)(0.205-x)Now, we need to determine if we can remove (–x) from the equation in the denominator. To do so, we need to determine the ratio of the initial concentration and Ka:initial concentrationK=0.2050.011=18<500Since the ratio is less than 500, we cannot neglect x. Calculating x using quadratic equation:Since the ratio is less than 500, we can’t remove (–x) from the equation. We first need to manipulate the equation to get a quadratic equation:0.011=(x)(x)(0.205-x)0.011=x2(0.205-x)x2+0.011x-0.00225We will then use the quadratic formula to solve for x. The quadratic formula is:x = -b±b2-4ac2aFrom the equation, we have a = 1, b = 2.08×10–3, and c = –4.0352 × 10–4. Solving for x, the equilibrium concentration of [H3O+] and [A–]:x = -b±b2-4ac2ax = 0.-0533 or x = 0.0423We take the positive value of x since the concentration of H3O+ and A– must increase. This means [H3O+] = [A–] = x = 0.0423 MCalculating the pH:pH = -log[H+]pH = -log(0.0423)pH = 1.374Therefore, the pH of the solution is 1.37

Problem: Find the pH of a 0.205 M HClO2(aq) solution. For HClO2, Ka =0.011.

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Problem Details

Problem: Find the pH of a 0.205 M HClO2(aq) solution. For HClO2, Ka =0.011.

FREE Expert Solution

Problem Details

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