In the titration of 77.5 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 10-4), with 0.38 M HCl, calculate the pH under the following conditions. (a) after 50.0 mL of 0.38 M HCl has been added (b) at the stoichiometric point
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Consider 67.0 mL of a solution of weak acid HA (Ka = 1.00 10-6), which has a pH of 4.500. What volume of water must be added to make the pH = 5.000?
Business management class
On finding the proper correct answer. It's easier too First read test booklet. The answers will most of the time will be there.( Note I was only checking meanings ver's difinations with booklet & Google Online for proper choice.) Business Management as far being dificu...
E4-19 On December 31, the adjusted trial balance of Oslo Employment Agency shows the following selected data. Accounts Receivable $24,000 Commission Revenue $92,000 Interest Expense 7,800 Interest Payable 1,500 Analysis shows that adjusting entries were made to (1) accrue $4,5...
which of the following effects would also occur at the end of an Ice Age 1.) an increase in volcanic activity near the equator. 2.) a global rise in the sea level. 3.) a worldwide extinction of the reptiles. 4.)a shorte length of the day. 5.)a complete rearrangement of the ear...
At a particular temperature, Kp = 0.25 for the following reaction. N2O4(g) 2 NO2(g) (a) A flask containing only N2O4 at an initial pressure of 5.3 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. (b) A flask containing only NO2 at ...
At a particular temperature, K = 1.00 102 for the following reaction. H2(g) + I2(g) 2 HI(g) In an experiment, 1.23 mol H2, 1.23 mol I2, and 1.23 mol HI are introduced into a 1.00 L container. Calculate the concentrations of all species when equilibrium is reached.
At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) SO3(g) + NO(g) If all four gases had initial concentrations of 0.580 M, calculate the equilibrium concentrations of the gases.
At a certain temperature, 4.0 mol NH3 is introduced into a 2.0 L container, and the NH3 partially dissociates by the reaction. 2 NH3(g) N2(g) + 3 H2(g) At equilibrium, 2.0 mol NH3 remains. What is the value of K for this reaction?