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Do the reagent for this type of addition reaction is the hygrogen halide for example HCl, HBr, HI or HF.
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- Which of the following is not used to be standardized against KHP? a. H2SO4 b. NaOH c. NH3 d. NH4A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid 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 perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.Calc solubility 2
- If NaOH(ag) is mixed with KNO3(ag) would a precipitate form? O Yes O NoA 1.00 liter solution contains 0.36 moles hydrocyanic acid and 0.28 moles potassium cyanide. If 0.14 moles of hydrochloric acid 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 hydrochloric acid.) ✓ A. The number of moles of HCN will decrease. True B. The number of moles of CN will increase. False C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HCN] [CN] will increase.3a) A student determines the concentration of a sodium hydroxide solution by titration with standardized KHP. S/he obtains the values: 0.190 M, 0.202 M, and 0.205 M. Should the value 0.190 M be rejected? Apply the Q Test. For three values Q must be greater than 0.94 to reject the number. Q = suspect nearest | largest - - smallest b) The student de to repeat the experiment two more The five values now include: 0.190 M, 0.202 M, 0.205 M, 0.201M and 0.203M. Use the Q Test to see if the first value may be rejected. For five values Q must be greater than 0.64 to reject the number. c) Solve for the average Molarity of the measurements from part b with and without the rejected number. Is there value in repeating an experiment several times?
- The solubility (denoted as s) of CaSO4 in pure water at 40o C is 1.09 grams per liter. What is the value of the solubility product of CaSO4?47. Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the vol- ume of each unknown HCl solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the con- centration (in M) of the unknown HCl solution in each case. HCI Volume (mL) NaOH Volume (mL) [NaOH] (M) 0.1231 M 0.0972 M 0.1178 M 0.1325 M a. 25.00 mL b. 15.00 mL c. 20.00 mL d. 5.00 mL 28.44 mL 21.22 mL 14.88 mL 6.88 mLA sample of 1.25 L of HCl gas at 21 °C and 0.950 atm is bubbled through 0.500 L of 0.150 M NH3 solution. Calculate the pHof the resulting solution assuming that all the HCl dissolves and that the volume of the solution remains 0.500 L.
- The molar solubility of zinc phosphate in a 0.172 M potassium phosphate solution is ___ M.What is the name of the process by which a solute dissolves in a solvent? OA. Precipitation B. Dissociation C. Ionization OD. SolvationAn analyst was titrating a solution of unknown acetic acid concentration with 0.01 M NaOH using phenolphthalein as indicator. After adding exactly 39.4 ml of the titrant drop-wise, the analyte solution started to turn light pink. The titrant volume 39.4 ml is best referred to as the O equivalence point. Onone of the choices O standardization point. O equilibrium point. O endpoint.