Calculate the moles of KHP titrated in each trial = M xL = 0.5 M x 0.025 L=_ Calculate the moles of NaOH using stoichiometry of the reaction

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the total solution volume (in mL) at the equivalence point? (Nearest whole number)

A solution contains 1.37x10-2 M zinc nitrate and 1.29x10-2 M barium acetate. Solid sodium carbonate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of carbonate ion when this precipitation first begins? [CO3²-] = M

An aqueous solution contains .15 M Cl* and .45 MT. A chemist wishes to do a fractional precipitation experiment in which he slowly adds Pb²*, which can form ppts of PbCl2 (s) [Ksp = 1.6 x 10-5] and Pbl2 (s) [Ksp = 8.4 x 10°]. Which of the following is entirely correct? Pb2+ .15 M .45 M CI- I-

A solution contains 1.18×102 M sodium carbonate and 9.93x10-3 M potassium sulfate. Solid silver nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of silver ion when this precipitation first begins? [Ag*]=| M

Be sure to answer all parts. Radiochemical techniques are useful in estimating the solubility product of many compounds. In one experiment, 50.0 mL of 0.080 M AgNO3 solution containing a silver isotope with a radioactivity of 74,025 counts per min per mL were mixed with 300.0 mL of a 0.040 M NaIO, solution. The mixed solution was diluted to 500.0 mL and filtered to remove all of the AgIO, precipitate. The remaining solution was found to have a radioactivity of 44.4 counts per min per mL.. What is the Ksp of AgIO,? x 10 (Enter your answer in scientific notation.)

If there was a mixture between Ba2+ and Ni2+. propose an anionthat could be added to that mixture to selectively precipitate only one of the remaining cations. Ifthis anion was added to this mixture, which cation will form a precipitate, and which cation willremain in solution?

I titrate a 5.00mL aliquot of Arsenic acid with 36.09 mL 0.126M sodium hydroxide. Calculate the molarity of the arsenic acid sample.

Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a  2.0 M NaI solution.  (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?