what is the concentration of both H30+ of 1.0x10-5 M Solution HCl + NaOH >> H2O

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Explanation / Answer

HCl + NaOH >> H2O + NaCl first try to convert your quantities of HCl and NaOH into moles. you have 50 ml of 0.1 M HCl 50 ml * (1 L / 1000 ml) = 0.05 L * 0.1 Mol / L = 0.005 mol HCl you have 50 ml of 0.1 M Naoh 50 ml * (1 L / 1000 ml) = 0.05 L * 0.2 Mol / L = 0.01 mol NaOH The chemical equation uses equal amount of mols of both HCl and NaOH, So since you have 0.01 mol NaOH and only 0.005 HCl, they will react and there will still be 0.005 mol NaOH remaining. The NaOH will dissociate in the water into the ions Na+ and OH-. The dissociation is just NaOH >> Na+ + OH- Since the coefficients are all 1, there is 0.005 mol of Na+ ions and 0.005 mol of OH- ions. the pOH = -log [conc of OH-] pOH = 2.3 and you know from the autoionization of water that, pH + pOH = 14 pH + 2.3 = 14 pH = 11.7 and then [H+] = 10^ (-pH) so [H+] = 2 * 10 ^ (-12) are you sure its 2 * 10 ^ 13 and not 12? in any case thats how you do it. hope that helps

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