Calculate the pH of a solution that is 0.27M in naOBr. Ka (HOBr) = 2.0x10^-9, include a balanced equation for the ion effecting the PH of this solution in water. detailed explaination please.
Calculate the pH of a solution that is 0.27M in naOBr. Ka (HOBr) = 2.0x10^-9, include...
The pH of 0.40M hypobromous acid (HOBr) is 5.05 a. Calculate the Ka and the % dissociation of the acid? b. what is the % dissociation if the salt 0.40M NaOBr is also present the above solution?
Calculate the pH and % dissociation of a 4.68 M solution of KOBr in water (ka=2.8*10^-9 for HOBr)
QUESTION 2 The K a of hypobromous acid, HOBr, is 2.6'10-9. Calculate the pH of a solution which is composed of 0.40 M HOBr and 0.40 M NaOBr. a. 9.12 b. 4.49 C. 8.59 d. 0.40 e. 0.80
what is the ph of a 0.27 M NaOBr solution? Acid. Ka HC2H3O2. 1.8x10^-5 C6H5COOH. 6.5x10^-5 CH2CICOOH. 1.4x10^-3 HOBr 2x10^-9 C6H8O6. 8x10^-5 HOI. 2.3x10^-11 answer options: A) 1.88 B) 0.57 C) 2.43 D) 12.12 E) 11.07 F) 13.43
Consider the following acids and bases: HCO2H Ka = 1.8 × 10-4 HOBr Ka = 2.0 × 10-9 (C2H5)2NH Kb = 1.3 × 10-3 HONH2 Kb = 1.1 × 10-8 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. (Select all that apply.) HONH2 KHCO2 HCO2H (C2H5)2NH (C2H5)2NH2Cl HOBr NaOBr HONH3NO3
Calculate the pH of the solution made by adding 0.50 mol of HObr in 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HObr is 2.0 * 10^-9
Find the pH of a 0.183 M aqueous solution of hypobromous acid (HOBr), for which Ka = 2.06 × 10–9.
Please explain the mechanism to me as well.
Part A Calculate the pH of the solution made by adding 0.50 mol of HOBr and 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HOBr is 2.0 x 10-9. Express your answer numerically using two decimal places. ► View Available Hint(s) O ADD A O O ? pH = Submit Request Answer
The Ka for HOBr is 2.8 x 10 ^-9. You titrate 20.0 mL of a 0.400 M HOBr solution using a 0.400 M NaOH. What is the pH after 10.0 mL of NaOH have been added (1/2 equivalence pt) and after 22.0 mL of NaOH have been added (overshot endpoint)? pH after 10.0 mL of 0.400 M NaOH = pH after 22.0 mL of 0.400 M NaOH = (total volume = 42.0 mL)
3) Hypobromous acid (HOBr) is a weak monoprotic acid, with Ka = 2.1 x 10^-9 . a) What is the value for pH for a 0.0424 M aqueous solution of hypobromous acid? [12 points]