how to find how many moles are needed to neutralize?
315636
['Step 1: Calculate the number of moles of OH-.', 'Molarity = moles/volume.', 'moles = Molarity x Volume.', 'moles OH- = 0.02 M/100 milliliters.', 'moles OH- = 0.02 M/0.1 liters.', 'moles OH- = 0.002 moles.']
1336772
divide 345 grams by molar mass which is 44 . 01 grams per mole to give the number of moles. 1 mole contains 6.022 x 10^23 molecules.
82071
Divide Grams by Grams per Mole Divide the number of grams of each reactant by the number of grams per mole for that reactant. 50.0 g of Na are used in this reaction, and there are 22.990 g/mol. 50.0 ÷ 22.990 = 2.1749.
832678
['Balance the chemical equation for the chemical reaction.', 'Convert the given information into moles.', 'Use stoichiometry for each individual reactant to find the mass of product produced.']
931927
The neutralization equation of HCl + NaOH gives you H2O + NaCl is already balanced because there are two moles of H on both sides, one mole of Cl on both sides, one mole of Na on both sides, and one mole of O on both sides.
27090
Normality of H2SO4= Molarity x 2 =0.1584 x2 =0.3168 N, since H2SO4 is dibasic. Volume of NaOH required to neutralise 258.2 ml. of H2SO4 =258.2 x 0.3168 / 0.4216 = 194.0 ml.
1373559
6 =9 milliequivalents (mEq) of acid . Hence we will need 9 mEq of a base for a complete neutralization ,and we must get them from a 0.1N NAOH solution. Since 1 ml of this base solution contains 0.1 mEq, 9/0.1 =90 ml are needed.
859926
Step 1: List the known quantities and plan the problem. to calculate the molality of the solution. Then use the molality equation to calculate the moles of solute. Then divide the grams of solute by the moles to determine the molar mass.
418552
['Determine how many grams are given in the problem.', 'Calculate the molar mass of the substance.', 'Divide step one by step two.']
124390
So 1 M H2SO4= 1 x 2= 2N. Normality bof NaOH=Molarity x 1. So 1 ml. of 2N (1M) H2SO4 is required to neutralise 2 ml.
330769
['If 1 mole of HCl or NaOH gives you 1 mole of H2O , then the number of moles in H2O is: [ 1÷1×1 ] = 1 mole.', 'Now you have to find out the molar mass (M) of water ( H2O ). ... ', 'Therefore the molar mass (M) of H2O is: ... ', 'Last step, find the mass (m) of water.']
898263
To calculate the moles of solute you will need to divide the weight in grams you have added to the solution by the weight in grams of one mole. For this example, use sodium chloride: NaCl. The weight of one mole, rounded to the nearest tenth, is the atomic weight of sodium, 23g, plus the atomic weight of chorine, 35.5.
1046076
Then use the molality equation to calculate the moles of solute. Then divide the grams of solute by the moles to determine the molar mass.
302356
Divide the number of grams of each reactant by the number of grams per mole for that reactant. 50.0 g of Na are used in this reaction, and there are 22.990 g/mol. 50.0 ÷ 22.990 = 2.1749.
478231
Divide Grams by Grams per Mole Divide the number of grams of each reactant by the number of grams per mole for that reactant. 50.0 g of Na are used in this reaction, and there are 22.990 g/mol.
547927
Divide the mass of your anhydrous (heated) salt sample by the molar mass of the anhydrous compound to get the number of moles of compound present. In our example, 16 grams / 160 grams per mole = 0.1 moles. Divide the mass of water lost when you heated the salt by the molar mass of water, roughly 18 grams per mole.
1382198
First the ideal gas law will be used to solve for the moles of unknown gas . Then the mass of the gas divided by the moles will give the molar mass. Step 2: Solve. Now divide g by mol to get the molar mass.