Molarity = mols of solute/L of solution
.1004 = mols of NaOH/.01864
moles of NaOH = .00187
Moles of NaOH = Moles of KHP
Now, multiply .00187 by the molar mass of KHP
.00187*204.22 = .38 g KHP
How many grams of KHP are needed to exactly neutralize 36.7 mL of a 0.328 M barium hydroxidesolution
This is not a possible compound. Please state the chemical name of this Potassium-Hydrogen salt of 'WHAT" accurately.
7.5 grams are needed because each milliliter is 1.50 grams, to get 5.00 mls, the calculation would be 5x1.50=7.5.
HCl has a molar mass of 36.461 grams per mole. This means that 72.922 grams of HCl are needed per liter of water to make a solution that has a concentration of 2M.
how many grams of calcium nitrate are needed to make a 500ml volume of a .5 molar solution
The answer is 7,5g.
I suppose that this solution doesn't exist.
93,31 g MgCl2 are needed.
The needed mass is 35,549 g.
The answer is 3,211 g.
If your solution is a total of 414g and 3.06% of it needs to be NaCl, then you just take 414 x .0306 = grams of NaCl. The rest of the grams will be from other species in the solution.
58 milligrams of NaCl are needed.
Molarity = moles of solute/Liters of solution 3 M KBr = moles KBr/1 liter = 3 moles KBr (119 grams/1 mole KBr) = 357 grams needed
Molarity = moles of solute/volume of solution 1.50 M = X Moles/125ml = 187.5 millimoles, which is 0.1875 moles The molar mass of CaCl2 = 110.98 grams 0.1875 moles CaCl2 (110.98g/1mol) = 20.8 grams needed
302 g sucrose are needed.
Weight to volume solution is calculated by the weight of the solute in grams divided by the volume of the solution in milliliters. Assuming that the solvent is water, then then 100 grams of glucose is needed.
124,9 g grams of ammonium carbonate are needed.
Balanced equation first. HNO3 + NaOH >> NaNO3 + H2O Now, Molarity = moles of solute/volume of solution ( find moles HNO3 ) 0.800 M HNO3 = moles/2.50 Liters = 2 moles of HNO3 ( these reactants are one to one, so we can proceed to grams NaOH ) 2 moles NaOH (39.998 grams NaOH/1mole NaOH) = 79.996 grams of NaOH need to neutralize the acid. ( you do significant figures )
Put 100 grams in a beaker and and around 500 mls of water until it dissolves, then top up the beaker to a liter. That is your 10% solution. The percentage solution is a ratio of the weight of the compound to the weight of the final solution.
Grams NaOH?? Balanced equation. 2NaOH + H2SO4 --> Na2SO4 + 2H2O 4.9 grams H2SO4 (1 mole H2SO4/98.086 grams)(2 mole NaOH/1 mole H2SO4)(39.998 grams/1 mole NaOH) = 4.0 grams NaOH needed =================
400 mls would require 40g of glucose for a 10% solution and thus 20g for a 5% solution.
More than 91 grams of potassium nitrate for 100 mL water.
2.5 mol/L x 1.500 L x 36.5 g/mol = 137 grams
First.Molarity = moles of solute/Liters of solution0.22 M HCl = X moles/1.0 L= 0.22 moles HCl--------------------------Second.0.22 moles HCl (36.458 grams/1 mole HCl)= 8.0 grams hydrochloric acid needed===========================