Which of the following is the strongest acid?
Group of answer choices
hypoiodous acid (molar mass: 143.89 g/mol; Ka = 2.0 x 10-11)
acetic acid (molar mass: 60.05 g/mol; Ka = 1.8 x 10-5)
nitrous acid (molar mass: 47.01 g/mol; Ka = 4.6 x 10-4)
chloroacetic acid (molar mass: 94.49 g/mol; Ka = 1.4 x 10-3)
chlorous acid (molar mass: 68.46 g/mol; Ka = 1.1 x 10-2)
What is the concentration of [OH-] in pure water if Kw = 6.97 x 10-15?
Group of answer choices
8.35 x 10-8 M
2.70 x 10-7 M
9.42 x 10-8 M
1.46 x 10-7 M
3.01 x 10-7 M
1)
Ka is acid dissociation constant.
Greater value of Ka implies, stronger acid.
ka is largest for chlorous acid
So, this is strongest
Answer: chlorous acid
2)
Kw = [H+] [OH-]
Since water is neutral, [H+] = [OH-]
So,
Kw = [OH-][OH-]
Kw = [OH-]^2
6.97*10^-15 = [OH-]^2
[OH-] = 8.35*10^-8 M
Answer: 8.35*10^-8 M
Which of the following is the strongest acid? Group of answer choices hypoiodous acid (molar mass:...
Which of the following is the strongest acid? chloroacetic acid (molar mass: 94.49 g/mol; Ka = 1.4 x 10-3) formic acid (molar mass: 46.03 g/mol; Ka = 1.8 x 10-4) propionic acid (molar mass: 74.08 g/mol; Ka = 1.3 x 10-5) hypoiodous acid (molar mass: 143.89 g/mol; Ka = 2.0 x 10-11) acetic acid (molar mass: 60.05 g/mol; Ka = 1.8 x 10-5)
All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+, NH3 CH3COOH, CH3COO- H3O+, OH- HPO42-, PO43- The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid? Group of answer choices 4.7 x 10-5 4.1 x 10-7 3.4 x 105 2.4 x 10-4 1.3 x 10-5 You have 250.0 mL of a 0.56 M solution of NaCH3COO. How many milliliters of a 0.50...
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...
7. How many grams of chlorous acid must be dissolved in water to make 100 mL of a HClO2 solution whose pH is 2.40? Ka for HClO2 = 1.1 x 10-2. Molar mass of HClO2 = 68.5 g/mol.
5B. (10 pts) If 2.846 g of pure chloroacetic acid (CHCICOOH. molar mass = 94.45 g/mol) is dissolved into water and then titrated with 0.7652 M NaOH (see the reaction below). What volume of the titrant NaOH will be required to reach the end point. CHCCOOH(aq) + NaOH(aq) + NaCH2CHCOO(aq) + H2O
please explain? Which of the following is the strongest acid? carbonic acid (Ka= 4.3 x 10-7) acetic acid (Ka= 1.8 x 10-5) boric acid (Ka= 7.3 x 10-10) lactic acid (Ka= 8.4 x 10-4). phenol (Ka= 1.3 x 10-10).
Which of the following acids is the strongest? O Acid A, Ka = 3.2 x 10-10 O Acid B, Ka = 6.4 x 10-14 O Acid D, Ka = 3.9 x 10-7 O Acid C, Ka = 4.2 x 10-5
Question 13 1 Point Which of the following is the strongest acid? Select the correct answer butanoic acid, CH3CH2CH2COOH (Ka = 1.51 x 10-6) hydrocyanic acid, HCN (Ka = 6.31 x 10-6) hydrofluoric acid, HF (Ka = 6.76 x 10-4) thiocyanic acid, HSCN (Ka = 12.59)
Be sure to answer all parts. A 0.1276 sample of a monoprotic acid (molar mass = 1.10 x 10 g/mol) was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH. After 10.0 mL of base had been added, the pH was determined to be 5.67. What is the K, for the acid? x 10 (Enter your answer in scientific notation.)
HELP! Part B: Determination of acid ionization constant (K.) and molar mass of an u Concentration of NaOH (mol/L) from bottle: 0.1053 Mass concentration of unknown acid (g/L) from bottle: 3.120 pH of unknown acid solution: 228 from pH meter. 1) Titration of unknown acid using indicator only Trial 2 Trial 1 1.593 30.851 090909 ml Mass of empty beaker Mass of beaker + unknown acid solution Mass of unknown acid solution Volume of unknown acid solution Initial volume of...