(b) If the titrant has a molarity of 0.1500 M and there are 40.00 mL of analyte present, what is the molarity of the analyte? 4.00.1500 X M (c) If 0.5256 g of analyte were dissolved in 40.00 mL of water to perform this titration, what is the molecular mass of the analyte? 4.01577 x g/mol

Consider a slightly soluble salt with a general form of MX2(s) --> M*(aq) + 2X(aq). If its molar mass is 121 g/mol and K, = 1.5 x 108, what is its solubility in grams per 100 mL? O 0.0015 g/100 mL O 0.019 g/100 mL O 0.15 g/100 mL O 0.55 g/100 mL,

How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M CuBr2 solution? CuBr2(aq) + 2KOH(aq) Cu(OH)2(s) + 2KBr(aq)g?

Consider the reaction of acetic acid (HC2H3O2) in vinegar with NaOH solution If 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point. What is the molarity of the vinegar solution? (Hint, write the balanced chemical reaction.) Also, what is the mass% of acetic acid in vinegar if the density of vinegar is 1.00 g/mL?

(b) (i) How many grams of NaOH are present in 53.0 mL of a 5.50 M solution?(ii) Calculate the volume in mL of a 1.420 M NaOH solution required to titrate 50.00 mL of a4.50 M H 2 SO 4 solution

In titrating a H2SO4 solution, it was found that 23.66 mL of 0.2137 M NaOH would neutralize 22.04 mL of the acid.  Find the molarity of the acid solution. (Note that this is not 1:1)               unit:

A student determined the concentration of NaOCI in a commercial bleach sample using the same technique described in section "F" of the Halogens and Their Compounds lab. The student required 18 drops of 0.01M Na,S203 to reach the end point. What is the concentration (reported in molarity) of NaOCI in the bleach sample?

In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH.  What was the molarity of the acetic acid solution?

40.00 mL of a solution of MgCl2 with a molar volume concentration of 0.933 mol/L is mixed with 100.0 mL of a solution of AlCl3 with a molar volume concentration of 0.211 mol/L.  What is the final molar volume concentration of chloride ions (Cl-) in the mixture in mol/L? Note: The density of pure water is 1.000 g/mL.

5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant Clic)