An experiment was carried out as follows: 1.5766 g of an ammonium salt was placed in a beaker and 60 ml of 1.182 M sodium hydroxide was added. The resulting mixture was heated for about an hour and then left to cool to room temperature. The reaction mixture was then titrated with sulfuric acid and required 18.35 ml of the acid for complete neutralization. Given that the percentage by mass of ammonium in the salt was 37.5 %, calculate the molarity of the sulfuric acid used in the titration.

A 25.00-mL sample of a commercial vinegar is diluted with de-ionized water to 100.0 mL. Then, a 10.00-mL portion of the dilute vinegar solution is titrated with 0.1125 M NaOH solution, and the titration requires 18.50 mL of the NaOH solution to neutralize the acetic acid in the dilute vinegar sample. Calculate the molar concentration of acetic acid in the original vinegar sample (before dilution). The acid-base reaction occurs as follows:              HC2H3O2(aq)  +  NaOH(aq)  -->  NaC2H3O2(aq)  +  H2O(g)          (A) 0.8325 M           (B) 0.2081 M           (C) 0.3330 M           (D) 0.2432 M

An aqueous solution of perchloric acid is standardized by titration with a 0.172 M solution of calcium hydroxide.If 30.0 mL of base are required to neutralize 19.3 mL of the acid, what is the molarity of the perchloric acid solution?

A 10.0 mL sample of an HCl solution is titrated with a 1.00 M NaOH solution. The neutralization reaction is complete when 2.45 mL of NaOH is added. What is the concentration of the HCl solution (in M)?

An aqueous solution of potassium hydroxide is standardized by titration with a0.174 M solution of hydrochloric acid. If 19.1 mL of base are required to neutralize 10.8 mL of the acid, what is the molarity of the potassium hydroxide solution?

A student needs to dilute a 0.47 M Pb(NO3)2  solution to make 77.0 mL of 0.22 M Pb(NO3)2. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.47 M Pb(NO3)2 solution that is needed.

An aqueous solution of hydroiodic acid is standardized by titration with a 0.165 M solution of calcium hydroxide. If 12.8 mL of base are required to neutralize 14.9 mL of the acid, what is the molarity of the hydroiodic acid solution? M hydroiodic acid

1 A 185.0 mL sample of 1.200 M Pb(NO3), is mixed with 73.50 mL of 1.500 M NaCl, and the PbCl, precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr, precipitate is also collected and dried. What is the mass (in grams) of the PbBr, precipitate, assuming the yield in each precipitation step is 100%? F1 Q 2 F2 W 211 # 3 80 F3 E $ 4 NOV 20 a F4 R 475 % F5 T A 6 tv ♫ c F6 Y Ⓒ & 7 Ni F7 U 8 DII F8 ZA | ( 9 C

An aqueous solution of sodium hydroxide is standardized by titration with a 0.119 M solution of hydroiodic acid. If 26.4 mL of base are required to neutralize 15.5 mL of the acid, what is the molarity of the sodium hydroxide solution? M sodium hydroxide

An aqueous solution of sodium hydroxide is standardized by titration with a 0.123 M solution of hydrobromic acid. If 24.6 mL of base are required to neutralize 10.8 mL of the acid, what is the molarity of the sodium hydroxide solution? M sodium hydroxide