0.30 moles of NaOH is added to 0.80 mole of weak acid HX. The resultant solution has pH 5.25. Calculate Ka for HX.
A. 3.4 x 10^(-6)
B. 9.4 x 10^(-6)
C. 6.5 x 10^(-5)
D. 2.4 x 10^(-5)
E. 1.6 x 10^(-6)
0.30 mol of NaOH and HX reacts to form 0.30 mol of NaX
moles of HX remaining = 0.80 - 0.30 = 0.50 mol
use:
pH = pKa + log {[conjugate base]/[acid]}
pH = pKa + log {[X-]/[HX]}
5.25 = pKa + log {0.30/0.50}
pKa = 5.472
use:
pKa = -log Ka
5.472 = -log Ka
Ka = 3.4*10^-6
Answer: A
0.30 moles of NaOH is added to 0.80 mole of weak acid HX. The resultant solution...
Acid HX is a weak acid with Ka = 1.0 x 10–6 . A 50.0 mL sample of 1.00 M HX(aq) is titrated with 1.00 M NaOH(aq). What is the pH of the solution at the points listed below during the titration? For each question, write the letter of the correct choice from the choices given below. A) 0.0 B) 1.0 C) 3.0 D) 6.0 E) 6.6 F) 7.0 G) 8.0 H) 9.85 I) 12.0 J) 13.0 12. Before any...
Part 3: Weak-Strong Titrations II. Experiment 2: 20.0 mL of 0.100 M HX (unknown, monoprotic acid) is being titrated with 0.250 M KOH. The Ka has been experimentally determined to be 5.62 x 10-6. A. Point A: 3.0 mL of the titrant has been added. 1. How many moles of HX are in your initial sample? _____________ 2. How many moles of KOH have been added? _____________ 4. How many moles of OH- have been added? ...
20. If 10 mL of 0.05 M NaOH is added to a 20 mL solution of 0.1 M NaNO2 and 0.1 M HNO2, what will be the pH of the resultant solution? Assume that volumes are additive. Ka for HNO2 = 7.1x10-4. 21. At 25°C, 50.0 mL of 0.50 M NaOH(aq) is added to a 250 mL aqueous solution containing 0.30 M NH3 and 0.36 M NH4Cl. What is the pH of the solution after the addition of the base?...
If 0.0751 moles of NaOH is added to 1.00 liters of 0.130 M CH3COOH (acetic acid), what will the pH of the resulting solution be? Ka of that acid is 1.8x10 5.25 5.11 4.60 4.25 4.89
Please give your pH answers to two decimal places. A 100.0mL 0.100M weak acid solution is titrated with a 0.100M NaOH solution. If the acid has a Ka of 3.4 x 10-5, what is the pH of the acid solution... Before any NaOH is added = At the equivalence point in the titration =
You are titrating a weak acid and after 40.0 mL of NaOH solution is added, the pH =4.00. After 60.0 mL more of the NaOH is added, the titration indicator turns color. What is the Ka of this acid ?
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
A titration of a 183.0 mL aqueous solution of 0.30 M HN3, a weak acid with a K of 1.9 x 10-5, with 0.18 M NaOH is performed. What is the pH of the solution after 78.0 mL of NaOH has been added (at 25°C)? 0 4.26 10.32 oo 6.91 4.83 Next DLL
Calculate the pH after 0.15 mole of NaOH is added to 1.07 L of a solution that is 0.59 M HNO2 and 1.05 M KNO2, and calculate the pH after 0.30 mole of HCl is added to 1.07 L of the same solution of HNO2 and KNO2. 0.15 mole of NaOH __________ 0.30 mole of HCl __________
A 0,05 M solution of a weak acid HX has a pH of 3.424, What is the Ka of HX?