Which solution has the highest pH?
0.065 M HIO (Ka=2.3x10-11) | |
3.5x10-4M HBrO (Ka=2.5x10-9) | |
5.2x10-7M C6H5NH2 (Kb=4.3x10-10) | |
1.2x10-7M HCl |
HIO, HBrO, HCl are acidic, therefore these substances will form low pH. C6H5NH2 is the base that will form the highest pH.
If you liked the answer, please rate it positively, you would help me a lot, thanks.
Which solution has the highest pH? 0.065 M HIO (Ka=2.3x10-11) 3.5x10-4M HBrO (Ka=2.5x10-9) 5.2x10-7M C6H5NH2 (Kb=4.3x10-10)...
Consider 0.10 M solutions following acids: HF, Ka = 6.8x10-4 HIO, K2 = 2.3x10-11 HC7H502, Ka = 6.3x10-5 HCOOH, K = 1.8x10-4 Which of the following statements is true? HC7H5O2 has the lowest pH and the largest percent dissociation. HF has the highest pH and the largest percent dissociation. HCOOH has the lowest pH and the largest percent dissociation. HIO has the highest pH and the smallest percent dissociation. HF has the lowest pH and HIO has the largest percent...
If the Ka of HBrO is 2.01 x 10-9, and the pH of a solution made from an HBrO and KBrO solution is 8.98. Determine the [KBrO] if the [HBrO] is 0.625 M.
The weak acid HIO has a Ka of 2.0×10−11. If a 1.7 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HIO(aq)+H2O(l)⇋H3O+(aq)+IO−(aq) Report your answer with two significant figures.
Which of the following 1.0 M solutions would have the lowest pH? Weak Base Weak Weink Ka Kb Acid HCN 4.9 x 10-10 HONH2 1.1 x 10-8 A) LINO3 HNO2 4.5 x 10-4 NH3 1.8 x 10-5 B) HONH3Br HIO 2.3 x 10-11 C6H5NH2 4.3 x 10-10 C) H2NNH3CIO4 HBrO 2.5 x 10-9 H2NNH2 1.3 x 10-6 D) Ca(Bro)2 CoH5COOH 6.3 x 10-5 C5H5N 1.7 x 10-9
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
What is the pH of a 0.100 M F- solution? ka(HF) = 6.8*10^-4 kb(F-) = 1.5*10^-11
Which 0.1 M solution of compounds below has the highest [H30*): formula Kb Name Hydroxylamine NH2OH 9.1x10-9 Isoquinoline C9H7N 2.5x10-9 Caffeine C8H10N402 4.1x10-4 Diethylamine (C2H5)2NH 6.9x10-4 Dimethylamine (CH3)2NH 5.9x10-4 O Diethylamine Hydroxylamine Isoquinoline Caffeine Dimethylamine
What is the pH of a 6.85 × 10−3 M weak acid solution, HA, if Ka = 4.5 × 10−6? Group of answer choices 1.2 4.8 9.1 3.8 6.5 What is the pOH of 4.50 × 10−4M HBr? Group of answer choices 10.7 6.7 1.7 12.3 3.3 What is the pH of a 9.67 × 10−3M solution of NaOH? Group of answer choices 13.0 4.6 12.0 9.4 2.0 A 6.5 × 10-2 M solution of a weak acid, HA, has...
Consider 1.0 L of a solution which is 0.45 M HF and 0.2 M NaF (Ka for HF = 7.2 x 10-4). Assume 2 significant figures in all of the given concentrations so that you should calculate all of the following pH values to two decimal places. Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on addition of HCl. Why do we need to convert to Kb? I know...
numbers 8-10 8. Determine the pH of a solution in which 1.00 mol H2C03 (Ka 4.2 x 10-) and 1.00 mole NaHCOs are dissolved in enough water to form 1,00 L of solution. 9. How many moles of NaHCO3 should be added to one liter of 0.100 M H2CO3 (Ka4.2x 10-7) to prepare a buffer with pH 7.00? 10) Determine the pH of 0.01 M NH3 (Kb= 1.8 x 10-5) when an equal volume of 0.05 M NH4Cl is added....