1. First, remember definition of M (moles), M = moles of species / L.
0.33 M = 0.33 moles HCl / L
2. Then, multiple your volume by the molar concentration:
0.33 moles HCl / L x 0.70 L = 0.231 moles HCl or you can say n=CONCENTRATION multiply by VOLUME(HCl) which gives 2310 mol HCl
It's helpful to carry the units with your calculations. That way you can check that numerators and denominators cancel to give you the units of your answer.
Molarity = moles of solute/liters of solution
or, for our specific purpose here
moles of solute (HCl) = liters of solution * Molarity
10 ml = 0.01 liters
moles of solute (HCl) = (0.01 liters)*(0.1 M HCl)
= 0.001 moles of HCl
------------------------------
moles = mass (g) / molar mass (g/mol)
So: 1.0 (g HCl) / 36.5 (g/mol HCl) = 0.027 mole HCl
That depends on the concentration (molarity) HCl, which is missing here.
0.03000 L x 1.000 mol/L = 0.03000 moles
0.23 mol
0.035mol
Molarity = moles of solute/Liters of solution (40 ml = 0.04 Liters) algebraically manipulated, Moles of solute = Liters of solution * Molarity Moles HCl = (0.04 Liters)(0.035 M) = 0.0014 moles HCl ==============
Molarity = moles of solute/Liters of solution ( 22.0 ml = 0.022 Liters ) moles of solute = Molarity * Liters of solution Moles of NaCl = 0.500 M * 0.022 Liters = 0.011 moles of sodium chloride -------------------------------------------
.0150 mol
0.29M = 0.29 moles in 1000 ml so 0.29 x 110/1000 = 0.0319 moles
Molarity = moles of solute/Liters of solution ( 20.0 ml = 0.02 Liters ) moles of solute = Liters of solution * Molarity 0.02 Liters * 0.800 M MgCl2 = 0.016 moles MgCl2 -------------------------------
The answer is 0,o276 moles.
The answer is 0,0509 mole.
5.50eq noob
Molarity = moles of solute/Liters of solution (40 ml = 0.04 Liters) algebraically manipulated, Moles of solute = Liters of solution * Molarity Moles HCl = (0.04 Liters)(0.035 M) = 0.0014 moles HCl ==============
The answer is 0,1 mol.
Molarity = moles of solute/Liters of solution ( 50.0 ml = 0.05 Liters ) 0.552 M KCl = moles/.0.05 liters = 0.0276 moles of KCl
Molarity = moles of solute/Liters of solution ( 22.0 ml = 0.022 Liters ) moles of solute = Molarity * Liters of solution Moles of NaCl = 0.500 M * 0.022 Liters = 0.011 moles of sodium chloride -------------------------------------------
.0150 mol
0.29M = 0.29 moles in 1000 ml so 0.29 x 110/1000 = 0.0319 moles
Molarity = moles of solute/Liters of solution ( 20.0 ml = 0.02 Liters ) moles of solute = Liters of solution * Molarity 0.02 Liters * 0.800 M MgCl2 = 0.016 moles MgCl2 -------------------------------
Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters ) 1.5 M KBr = moles KBr/0.025 Liters = 0.038 moles potassium bromide ------------------
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------