A 5.01 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.094 L of solution. If the pH of the solution is 2.60, what is the Ka of HY?
A 5.01 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.094 L...
A 4.57x10^-3-mol sample of HY is dissolved in enough H2O to form 0.085L of solution. Enter your answer in the provided box. A 4.57 x 103-mol sample of HY is dissolved in enough H2O to form 0.085 L of solution. If the pH of the solution is 2.25, what is the K of HY? к,
A 0.195-mol sample of HX is dissolved in enough H2O to form 645.0 mL of solution. If the pH of the solution is 4.30, what is the K, of HX? Be sure to report your answer to the correct number of significant figures. x 10 (Enter your answer in scientific notation.)
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
A 4.691 g sample of MgCl2 (95.21 g/mol) is dissolved in enough water to give 750.0 mL of solution. What is the chloride (35.45 g/mol) ion concentration (in molarity) in this solution?
A 5.00-gram sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 25 torr at 25
What is the Kb for methylamine, CH3NH2, if a solution prepared by dissolved 0.82 mol of methylamine in 425 mL of H2O has a pH of 12.46? (Ans: 4.4 x 10-4) A 0.100 M solution of formic acid, HCOOH, is 4.0% dissociated. Calculate Ka for formic acid. (Ans: 1.7 x 10-4)
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.
numbers 8-10 8. Determine the pH of a solution in which 1.00 mol H2C03 (Ka 4.2 x 10-) and 1.00 mole NaHCOs are dissolved in enough water to form 1,00 L of solution. 9. How many moles of NaHCO3 should be added to one liter of 0.100 M H2CO3 (Ka4.2x 10-7) to prepare a buffer with pH 7.00? 10) Determine the pH of 0.01 M NH3 (Kb= 1.8 x 10-5) when an equal volume of 0.05 M NH4Cl is added....
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.