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?

The maximum contaminant level of cyanide (CN) in drinking water as set by the the Environmental Protection Agency (EPA) is 0.00020 g · L. Express this concentration in parts per million (ppm). Assume the density of water is 1.00 g/mL. concentration: Ppm

6. A 0.4622-g sample of potassium hyd rogen phthalate was dissolved in 50 mL of deionized water and titrated to a phenolphthalein end-point with 19.48 mL of NaOH solution. What is the molarity of the NaOH? 7. Assuming that the density of vinegar is 1.012 g/m L, calculate the weight percent of acetic acid in vinegar if 23.85 mL of 0.1311 M NaOH was required to titrate 5.00 mL of vinegar. did HA nd dis 192 riw o asuuc no'noleauoetb s obulbo. As 900 900 4Coz2 anigll .asbtucf namheqx dini 209 (0 HoO Cag) (es) ibis 9C D DV 9 ballet tnabole A 9 u u 1oied qütenud orlf hi asiddud e 9t borsoog szib alddud sis ord nolt dsvawnlcrndtuodA 9l il blucwnolduloe HOe wans uoy nistqx3 Sipid oo! tstse : wot oo dhelom t bbs rg beau yilednobbos nsbile s est itbin ow osta isrl bsbne evicmi Srtulce HOs orts to yahelom orld ininetsb as 9 adant anoto toi n odslo 613 Exbiont Aorf

0.1061 g of dissolved oxalic acid dihydrate (molecular weight = 126.064 g/mole) is reacted with 20.0 mL of a sodium hydroxide solution. Calculate the molarity of the sodium hydroxide solution.  The balanced equation can omit the dihydrate from oxalic acid. Group of answer choices 0.0421 M 1.34 M 0.334 M 0.0842 M 0.669 M

If you added 45.5 mL of 0.058 M KMnO4, 35.6 mL of 0.6M NaOH, 75.4 mL of 0.8M Ca(OH)2, and43.5 mL of H2O (l), what is the final concentration of hydroxide ions (assume all volumes areadditive)?

Calculate the molarity of HCl in a solution, which was prepared by dissolving 5.5 g of HCl (molar mass = 36.46 g/mol) in 200 g of C2H60. The density of the solution is 0.79 g/mL.

+2 When excess Na,so, solution was added to 20.0 mL of an unknown solution containing Ca ion, 0.0472 g of Caso, precipitated. What is the molar concentration (molarity) of Ca in the unknown solution? (molar mass of Caso, = 136.14 g/mol A) 1.36 x 102 B) 2.47 x 102 C) 2.10 x 10 D) 1.73 x 10 E) 3.83 x 10 Select one: -2 O a. 2.47 x 10 -2 с. 3.83 х 10 d. 1.73 x 10 -2 е. 2.10 х 10

Calcium nitrate  (Ca(NO3)2 ; MM =164.0878 g/mol)) dissolves in cold water to the extent of 266 g per 100. mL.  What is the concentration (mol/L) of nitrate ions in this solution? Ca(NO3)2 -> Ca+2 + 2 NO3-

1. The following reaction occurs in your lab: You have 225.0 mL of 0.345 M Na3PO4. How many grams of precipitate can are made? Balanced Rxn: 3 CaCl2 (aq) + 2 Na3PO4 (aq) → 6 NaCl (aq) + Ca3(PO4)2 (s) - 2. How many mL of a 0.220 M solution of KOH will be required to titrate 38.00 mL of a 0.0566 M solution of H3PO4? Balanced Rxn: H3PO4 (aq) + 2KOH (aq) → K2HPO4 (aq) + 2H2O (1)

The concentration of magnesium ions in seawater is approximately 0.0541 M. To the solution in part 3 above with MgSO4•7H2O (Epsoms Salt), how many more grams of MgCl2•6H2O will you need to use to make 1.0 L of water with the same concentration of magnesium ions as seawater?     (I am reasking this question since the one I posted was never answered, how do I cancel the previous, duplicate question please?)