Determine the molar concentration of each ion present in the solutions that result from each of the following mixtures: (Disregard the concentration of H+ and OH- from water and assume that volumes are additive.)  121 mL of 0.64 M CaCl2 and 121 mL of 0.24 M CaCl2

write the balanced chemical equation for the reaction between phosphoric acid and iron(II) hydroxide.  Calculate the mass of precipitate that can be formed when starting with 15.79 mL of 0.091 M phosphoric acid.

If 55.0 mL of a 0.25M solution of Mg(OH)2 is spilt on the floor, what volume, in mL, of 0.15M HBr  is needed to neutralize the base?  2HBr(aq) + Mg(OH)2 --> 2H2O(l) + MgBr2(aq)

How many mL of 0.022 M HCl would it take to completely neutralize 14.11 mL of 1.16 M Ca(OH)2 according to the following reaction equation. 2HCl + Ca(OH)2 --> 2H2O + CaCl2

Determine the molar concentration of each ion present in the solutions that result from each of the following mixtures:(Disregard the concentration of H+ and OH- from water and assume that volumes are additive.) (a) 47.9 mL of 0.85 M HCl and 77.6 mL of 1.51 M HCl  M H+=       M Cl-= (b) 125 mL of 0.63 M CaCl2 and 125 mL of 0.22 M CaCl2  M Ca2+=  M Cl-= (c) 31.0 mL of 0.333 M NaOH and 22.7 mL of 0.241 M HCl M Na+=  M Cl-= M H+= M OH-=   (d) 10.4 mL of 0.602 M H2SO4 and 21.5 mL of 0.151 M NaOH  M Na+=  M SO42-= M H+= M OH-=

A 0.0250 L sample of hydrochloric acid is placed in a flask with a few drops of phenolphthalein indicator. If 0.0326 L of a 0.185 M sodium hydroxide solution is needed to reach the endpoint, what is the concentration (M) of the hydrochloric acid solution?

You are asked to double check the calculations for the % soda ash (Molar mass = 105.99 g/mol) in your sample. You have calculated the [NaOH] to be 0.10012 M and the [HCI] to be 0.1007 M. Your lab partner prepared the soda ash sample by adding 2.352 g of unknown into 748.0 mL of distilled water. You prepared the sample by adding 28.0 mL of soda ash, 55.0 mL distilled water, 4 drops of phenolphthalein indicator and you filled the burette with HCI. The initial reading of the burette was 0.56 mL. The pink solution turned colourless at 21.92 mL and your lab partner noted down the volume of 43.81 mL for the second inflection point. Looking at the following set up below, how many errors are present from the information presented above? [(0.1012 M) x (0.4325 L) x (1/2) x (105.99 g/mol)] 2.352 g r %Ca2+ x 100% 25.00 mL 748.0 mL)| 1 error 5 errors 2 errors 3 errors LJ.0U TIL [2.352 g z ( 748.0 mL O1 error 5 errors 2 errors 3 errors 0 errors 4 errors

A 22.47 mL sample of dilute HBr requires 31.92 mL of 0.117 M KOH for neutralization.  Determine the molar concentration of HBr in the sample

Use the References to access important values if needed for this question. The molarity of an aqueous solution of nitric acid, HNO3, is determined by titration with a 9.07 x 10-2 M potassium hydroxide, KOH, solution. HNO3 + KOH → KNO3 + H2O If 39.8 mL of potassium hydroxide are required to neutralize 27.8 mL of the acid, what is the molarity of the nitric acid solution? Molarity = M Submit Answer Retry Entire Group 4 more group attempts remaining

Solid ammonium carbonate is slowly added to 175 mL of a 0.406 M magnesium sulfite solution until the concentration of carbonate ion is 0.0108 M. The percent of magnesium ion remaining in solution is