Calculate the concentration of KCL in grams per liternofnsolution. Divided the mass of the KCL residue 1.433g by the initial volume of the KCL solution in mL 5mL and multiply by 1000. Record the resulting concentration 286.6g /mL

What do you understand about the manufacture of chemical solutions? How to (a) make 1000 mL of 0.2 N hydrochloric acid solution from 1 N standard solution and (b) make 100 mL of 0.5 N sodium hydroxide secondary standard solution (known BM = 40 g / mL)? Explain!

Calculate the number of grams of AgCl will precipitate out of solution if 125 mL of 0.500 M AgNO3 is combined with 275 mL of 0.235 M NaCl according to the following         AgNO3 (aq)   +    NaCl (aq)  -->  AgCl (s)   +  NaNO3 (aq)

Consider the following reaction. MgCl,(aq) + 2 NaOH(aq) – Mg(OH), (s) + 2 NaCI(aq) Calculate the volume of 0.169 M MgCI, that is needed to react completely with 80.5 mL of 0.450 M NaOH. 214 mL 429 mL 15.1 mL 107 mL

Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of citric acid to be 192.124 g/mol. Give your answer to one decimal place. initial volume (mL) final volume (mL) Buret reading (mL) 1.75 14.32

A student is asked to standardize a solution of barium hydroxide. He weighs out 0.929 g potassium hydrogen phthalate ( KHC8H404, treat this as a monoprotic acid). It requires 36.8 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the barium hydroxide solution? M This barium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 28.5 mL of the barium hydroxide solution is required to neutralize 13.3 mL of hydrobromic acid, what is the molarity of the hydrobromic acid solution? M

A student needs to dilute a 0.40 M Pb(NO3)₂ solution to make 75.0 mL of 0.16 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 0.40 M Pb(NO3)₂ solution that is needed. 75.0 mL 75.0 L Answer Bank 0.40 M 0.16 mL 0.16 M 0.40 mL = mL

1. A 10. mL portion of a 0.60 M CuSO:(aq) solution is diluted to a volume of 0.10 L. What is the final concentration of this solution? Identify M1, V1, M2, and V2.

Solid potassium hydroxide is slowly added to 175 mL of a 0.0631 M magnesium acetate solution. The concentration of hydroxide ion required to just initiate precipitation is М.

29.91 ml of an acid solution (identity unknown) is neutralized by 17.29 ml of 0.1999 M calcium hydroxide solution. Determine the Normality of the acid.