# Acid/Base Chemistry

posted by .

A 497 mL sample of 0.9960 M HI is mixed with 443 mL sample of KOH (which has a pH of 13.51). What is the pH of the resulting solution?

What are the steps to solving this problem? I think you need to find the concentration of OH by taking 10^-pOH, and then do an ICE table from there but I keep getting an incorrect answer. Thank you.

• Acid/Base Chemistry -

Hi is an acid; KOH is a base. They partially neutralize each other.
HI + KOH ==> KI + H2O
You are right. Find the OH^-.
mols HI = M x L = about 0.495
mols KOH = M x L = ?
Subtract to find the one in excess and
M = mols excess/total volume in L.
Then pH = -log(H^+) if HI in excess or
14-pOH = pH if OH in excess.

## Similar Questions

1. ### AP CHEM

Please help me with these AP Chemistry homework problems and show me the steps how to find the solutions: Liquid-Liquid Tirations: What is the concentration of the unkown solution for each of the following titrations?
2. ### college chemistry

Consider the titration of a 50.0 mL sample of a 0.100 M solution of the triprotic weak acid citric acid (H3C6H5O7) with 0.100 M KOH. For citric acid, the three (3) acid dissociation constant values are ka1 = 7.40x10-3, ka2 = 1.70x10-5, …
3. ### AP Chemistry

A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with …
4. ### chemistry

A 20ml sample of .125M diprotic acid solution was titrated with .1019M KOH.the constants for the acid are k1=5.2*10 ^-5 and K2=3.4*10 ^-10. What added volume of base does each equivalence point occur?
5. ### Chemistry

A 15.5 mL sample of 0.215 M KOH solution requires 21.2 mL of acetic acid in a titration experiment. Calculate the molarity of the acetic acid solution. Please show all steps, I don't understand this.
6. ### Chemistry

A sample of 30.0 mL of sulfuric acid solution was titrated with 0.720 M KOH. It was found that 46.9 mL of the base was needed to neutralize the acid. What is [H2SO4]?
7. ### Chemistry Lab

A 15.00 mL sample of a weak acid with Ka = 3.52x10-4, was titrated with 0.475 M KOH. The equivalence point was reached after addition of 19.5 mL of KOH with the phenolphthalein indicator. Determine the molar concentration of the original …
8. ### Chemistry

A sample of g 0.2050 oxalic acid (4.2 H2C2O H2O) required 25.52 mL of KOH solution to complete the neutralization according to rea tion: HOOCCOOH + 2 KOH + KOOCCOOK ↔ H2O Which the concentration in mol L-1 of this KOH solution?
9. ### Chemistry

A 349mL sample of 1.659 M HI is mixed with 511 mL sample of NaOH (which has a pH of 13.35). What is the pH of the resulting solution?
10. ### Chemistry

A 349mL sample of 1.659 M HI is mixed with 511 mL sample of NaOH (which has a pH of 13.35). What is the pH of the resulting solution?

More Similar Questions