If you titrate 25 mL of 0.15 M formic acid (HCOOH, Ka = 1.8x10–4) with 0.060 M NaOH, what would be the pH after addition of 15 mL of NaOH solution?
If you titrate 25 mL of 0.15 M formic acid (HCOOH, Ka = 1.8x10–4) with 0.060...
A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125 M NaOH solution. Ka of HCOOH = 1.7 x 10−4. a. Calculate the pH of the solution after 50 mL of NaOH solution has been added. b. How many mL of 0.125 M NaOH need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
A buffer made with 150.00 mL of 0.20 M formic acid (Ka=1.8x10-4) and 250.00 mL of 0.10 M formate has a final volume of 1.0 L. What is the pH after 6.00 mL of 1.0 M HCL is added to the buffer?
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point? You are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . If you add 20.00 of to the beaker before...
We’re going to titrate formic acid with the strong base, NaOH. There is initially 100. mL of 0.50 M formic acid and the concentration of NaOH is 1.0 M. What is the initial pH of the formic acid solution? 2) What is the percent ionization under initial conditions? 3) After the addition of 10 mL of NaOH, what is the pH? 4) After the addition of 25 mL of NaOH, what is the pH? Think about where in the titration...
Calculate the pH of a 0.0167 M aqueous solution of formic acid (HCOOH, K, = 1.8x10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH [HCOOH)equilibrium [HCOO equilibrium
25.0 mL of 0.10 M formic acid (HCOOH, Ka = 1.8 x 10-4) is mixed with 20.0 mL of 0.10 M potassium hydroxide. What is the pH of the resulting solution? A. 2.37 B. 4.35 C. 13 D. 0.60
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
1.0 L of a 1.2 M solution of formic acid (Ka=1.8x10-4) was prepared. What is the pH of this solution? 1.8328 You are correct. Your receipt no. is 162-1608 Previous Tries Enough potassium formate was added to achieve a final potassium formate concentration of 1.7 M (assume the volume does not change). What is the pH of this new solution? 3.8960 You are correct. ceipt no. is 162-6598 Previous Tries 10 mL of 10 M NaOH is added to the...
What is the pH of the solution when 100 mL of 0.8 M formic acid (Ka= 1.8x10-4) is titrated with 50 mL of 1.2 M NaOH? 1.80 grams of an unknown monoprotic acid (HA) required 48.62 mL of a 0.25 M NaOH solution to reach the equivalence point. Calculate the molar mass of the acid. Need help understanding please show work. Thank you in advance.
Calculate the pH of a 0.065 M formic acid (HCOOH) solution. Formic acid is a weak acid with Ka = 1.8 × 10–4 at 25°C. 2.48 is WRONG answer!!!!!! Write your answer to two decimal places. Calculate the pH of a 0.065 M formic acid (HCOOH) solution. Formic acid is a weak acid with 1.8x 10at 25°C. pH 2.48