A student determines that an aqueous solution that contains 0.196 M potassium fluoride and 0.206 M hydrofluoric acid, also has an H3O+concentration of 8.48×10-4 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium:
Calculate K as is usually done, omitting the
solvent, water, from the expression for K: K =
and
A student determines that an aqueous solution that contains 0.365 M potassium nitrite and 0.125 M nitrous acid, also has a H3O+concentration of 2.10×10-4 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium:
(1) as is usually done, without the inclusion of
water in the expression for K: K =
(2) for comparison, with the inclusion of water in
the expression for K: K =
A student determines that an aqueous solution that contains 0.196 M potassium fluoride and 0.206 M...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
A solution contains 0.231 M potassium fluoride and 0.120 M hydrofluoric acid. The pH of this solution is .
A solution contains 0.323 M potassium fluoride and 0.416 M hydrofluoric acid. The pH of this solution is .
An aqueous solution contains 0.483 M ammonia (NH3). How many mL of 0.206 M hydroiodic acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.090? mL
A 1.00 liter solution contains 0.34 M ammonia and 0.44 M ammonium bromide. If 0.110 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) _______TrueFalse A. The number of moles of NH3 will increase. _______TrueFalse B. The number of moles of NH4+ will remain the same. _______TrueFalse C. The equilibrium concentration of H3O+ will remain the same. _______TrueFalse...
1) In the laboratory, a student combines 32.6 mL of a 0.374 M zinc fluoride solution with 21.3mL of a 0.458 M silver fluoride solution. What is the final concentration of fluoride anion? 2) A 9.43 g sample of an aqueous solution of hydroiodic acid contains an unknown amount of the acid. If 29.7 mL of 0.450 M sodium hydroxide is required to neutralize the hydroiodic acid, what is the percent by mass of hydroiodic acid in the mixture? _____%...
The pH of an aqueous solution of 0.118 M
potassium fluoride,
KF (aq), is .
This solution is
_________acidicbasicneutral
Write the balanced NET IONIC equation for the reaction that
occurs when nitric acid and calcium
hypochlorite are combined. It is not necessary to include
states such as (aq) or (s).
+
+
This reaction is classified as: _________Strong Acid +
Strong BaseWeak Acid + Strong BaseStrong Acid + Weak BaseWeak Acid
+ Weak Base.
The extent of this reaction is: _________Below...
Q.1 (a) An aqueous solution of ethanol and acetic acid is heated to 100oC. Each substance has an initial concentration of 0.810 mol L-1. At equilibrium, the acetic acid concentration is 0.748 mol L-1. Calculate the value of the equilibrium, K, for the reaction. Equation C2H5OH(aq) + CH3CO2H(aq CH3CO2C2H5(aq) + H2O(l) Initial (M) Change (M) Equilibrium (M) 0.748 (b) Propose two methods that would result in an increased concentration of CH3CO2C2H5(aq).
The reaction between potassium dichromate and concentrated hydrochloric acid, produces a mixed aqueous solution of chromium(III) chloride and potassium chloride, and evolving gaseous chlorine. K2Cr2O7(s) + 14 HCl(aq) ⟶ 2 K+(aq) + 2 Cr3+(aq) + 8 Cl- (aq) + 7 H2O(l) + 3 Cl2(g) Suppose that 9.73 g of K2Cr2O7(s) react with concentrated HCl, and that the final volume of the solution is 124.3 mL. Calculate the final concentration of Cr3+(aq) produced: (Aside: also, think about and the number of...
1. A buffer solution contains 0.256 M hydrofluoric acid and 0.308 M potassium fluoride. If 0.0414 moles of hydrochloric acid are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydrochloric acid) pH = 2. A buffer solution contains 0.328 M ammonium chloride and 0.331 M ammonia. If 0.0396 moles of sodium hydroxide are added to 225 mL of this buffer, what is the...