Calculate the pH and % dissociation of a 4.68 M solution of KOBr in water (ka=2.8*10^-9 for HOBr)
Calculate the pH and % dissociation of a 4.68 M solution of KOBr in water (ka=2.8*10^-9 for HOBr)
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
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.
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)
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?
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
2. Calculate the pH, pOH, [H3O+], and [OH-] of a 0.30 M solution of the weak acid, hypobromous acid, HOBr. The Ka value for HOBr is 2.8 x 10-9.
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]
final answwr is [HOBr]= 0.0001 M, [OBr]= 0.0000037 M and [Br2]
= 0.000000183 M
10- mole of bromine, BI2, is added to a liter of water. The resulting pH is 7.0. Give equilibrium, n that the following reactions are at Br2 H20 H Br-HOB-6x10 HOBr H + + OBr7: Ka-3.7 x 10-9 and that [Br") = 1.1 × 10-4, including the Br-originally present in the sample, what are the molar concentrations of Br2, HOBr, and OBr?
10- mole of bromine,...
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