(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

800ml sample of 2.00 molar formic acid HCOOH (or HA) ismixed with 200ml of a 4.80 molar NaOH. Calculate the [H_{3}O^{+}] of the resulting solution.

2. Relevant equations

(for buffers) pH=pKa-log(HA/A^{-})

Ka for formic acid is 1.8x10^{-4}

pH=14-pOH

[H^{+}]=(1.00x10^{-14})/([OH^{-})

3. The attempt at a solution

Well, I used an ICE chart of formic acid with water to find the concentration of hydronium ions at equilibrium, which came out to be 1.7x10^{-2}M, and used some stoichiometry to figure out that there are 0.960 moles of NaOH, and thus, .960 moles of OH^{-}.I subtracted the amount of hydronium ions from the moles of hydroxide ions (since the total volume happens to be one liter), and found this to be my concentration of hydroxide ions, .943M. Using the formula above to calculate hydronium ion concentration from hydroxide ions and the ionization constant for water at 25 degrees celcius, which we assume this is at, I derived the concentration of hydronium ions to be 1.1x10^{-14}, which gives a pH of 13.97.

I was expecting a basic solution since there was so much hydroxide ions added, but this number just seems surreal. I appreciate any comments.

ICE Chart of Formic Acid:

HA + H_{2}O <--> A^{-}+ H_{3}O^{+}

I 1.6 0 0

C -x +x +x

E 1.6-x x x

(sorry it all got squished together, but to clear things up, the water column was left blank)

1.8x10^{-4}=(x^{2})/(1.6-x)

Assuming the x is negligabile to 1.6 gives us:

x=1.7x10^{-2}

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