2. At standard temperature and pressure, 5.6 L of H,S is dissolved in enough water to...
a. Enough of a monoprotic acid is dissolved in water to produce a 0.0163 M solution. The pH of the resulting solution is 2.51. Calculate the Ka for the acid. Ka= ________ It's not 5.86 10-4. I tried it and it wasn't correct. b. The Ka of a monoprotic weak acid is 6.61 × 10-3. What is the percent ionization of a 0.108 M solution of this acid? Percent ionization= ___________ it's not 24.72 %. I tried it's also incorrect.
Enough of a monoprotic acid is dissolved in water to produce a 1.06 M solution. The pH of the resulting solution is 2.56. Calculate the K, for the acid. Number If the K of a monoprotic weak acid is 7.1 x 10 what is the pH of a 0.40 M solution of this acid? Number PH- The K of a monoprotic weak acid is 2.57 x103. What is the percent ionization of a 0.178 M solution of this aci Number
Enough of a monoprotic weak acid is dissolved in water to produce a 0.0140 M solution. The pH of the resulting solution is 2.50. Calculate the Ką for the acid. Ka =
If 6.6 g of butanoic acid, C_4H_8O_2, is dissolved in enough water to make 1.0 L of solution, what is the resulting pH? A table with K_a values can be found here. pH =
when 0.45 moles of a weak acid are dissolved in enough water to make 0.800 L the pH of the resulting solution is 5.27. calculate Ka
We place 0.134 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.18 . Calculate the ionization contant, Ka, of HA
We place 0.133 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.23 . Calculate the ionization contant, Ka, of HA.
We place 0.118 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.29 . Calculate the ionization contant, Ka, of HA.
TML 4. Calculate the molarity when 40.0 g of sodium hydroxide is dissolved in enough water to make a 3.0 L solution. M= mol solute 40.09 Nao L soin 37. mi Calculate the more feilver nitrate in 185 ml of a 2.50 M solution.
At a temperature of 25.0◦C, we dissolve 3.33 g of an acid, HA, in enough water to produce 25.0 mL of solution. We titrate this solution with a 0.444 M NaOH solution and we require 18.8 mL to reach the equivalence point. The ionization constant of HA, Ka, is 5.5 × 10−6 . The temperature is 25.0◦C throughout. (a) (2 points) What is the molar mass of HA? (b) (2 points) What was the original pH of the HA(aq) solution?...