Ka = 2.5 times 10-9 for HOBr. The pH of 0.042 M Hypobromous acid (HOBr) is 5.07. Set up the equilibrium equation for the dissociation of HOBr. Calculate the value of the acid-dissociation constant. 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 * 10-9.

Question: 1st attempt Select the correct statements in regard to acid strength. Choose one or more: O HOBr is more acidic than HOBrO OHOBr is more acidic than HOC O HOCI is more acidic than HOB HOBrO is more acidic than HOBr

Hypobromous acid, HOBr, is a weak acid with a Ka = 2.5 x 10-9 (a) Calculate the pH of a 0.350 M aqueous solution of hypobromous acid. Clearly justify any approximation you make in your calculation. (b) Calculate the value of pKb, of the hypobromite ion, OBr". Give the chemical equation to which the pKb you have calculated refers.

Question: Molecules of gaseous hypobromous acid, HOBr(g), have one H–O bond and one O—Br bond: H-0— Br HOBr can react with H, to form H2O and HBO HOBr(g) + H2(g) → H2O(g) + HBr(9) AH = -216 kJ Using this equation and the data in the table, determine a value for the bond enthalpy of the O-Br bond in HOB. 177 kJ/mol 393 kJ/mol …

NBr_3 + NaOH → N_2 + NaBr + HOBr Balanced Equations: Balanced equations are those that have an equal number of atoms of an element that are present on either side of the respective equation.

Consider a 0.35 M solution of hypobromous acid (HOBr) in water. The equation for the dissociated of this weak acid is HOBr (aq) rightleftharpoons H^+ (aq) + OBr^- (aq) and k = 2.4 times 10^9. What is the HOBr (aq), H^+ (aq), OBr^- (aq) concentration at; 1) What is the pH of a 1.67 M solution of carbonic acid?

OBr^(-) + H2O arrow HOBr + OH^(-) Write the equation for the reaction of HSO3- with water in which it acts like a base and identify the acid, base, conjugate acid, and conjugate base. Identify the strongest acid, then write an express

Question: Step 1: ClO−+H2O→HOCl+OH Step 2 Br−HOCl→HOBr+Cr Step 3: OH+HOBr−→H2O+BrO− Convider the reaction mechanism. Part A: is this the concct everodl reaction? GACKGROUND ClO+Br→Cl−+BrO− Writing plausible reaction mechanikms: Sum of ritmentary steps MUST gove the overall balanced equation for the resction Part B: if the ...

The value of Ka for HOBr is 2.0×10−9. 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. There are 2 steps to solve this one.

The Ka for hypobromous acid, HOBr is 2.5 x 10^{-9}. What is the pH of a 0.11 M solution of the acid? What is the % ionization of the acid at this concentration? Hypobromous acid, HOBr, has an acid-ionization constant of 2.5 x 10-9 at 25 degrees Celsius. What is the hydronium ion concentration in a 0.57 M HOBr solution?