100.mL of 0.200 M HCl is titrated with 0.250 M NaOH.
What is the pH of the solution at the equivalence point?.
2007-03-13 14:56:52 · 3 answers · asked by xo_cristina_xo 1 in Science & Mathematics ➔ Chemistry
At the equivalence point you have equal moles of OH- and H+, so your pH is 7.
2007-03-13 15:00:56 · answer #1 · answered by chemmie 4 · 1⤊ 0⤋
volume of moles or equivalents are equivalent. If the two the acid and the backside have purely one ionizable hydrogen (for the acid) or hydroxide (for the backside) then the equivalence element is the place the moles are equivalent. Liters x Molarity = Moles (for the reason that Molarity = Moles consistent with Liter) mL x M = millimoles. 2 equations you will use are- L x M = L x M L x M = grams/molecular weight (moles) in case you have an acid like H2SO4, then the equivalent weight is a million/2 of the molecular weight so the normality (N) = 2 x Molarity.
2016-11-25 01:41:56 · answer #2 · answered by Anonymous · 0⤊ 0⤋
Strong acids and bases neutralize each other completely at pH7.
2007-03-13 15:00:36 · answer #3 · answered by cattbarf 7 · 0⤊ 0⤋