C1V1 = C2V24 x .04 = 1 x V2V2 = (4 x .04)/1= 160mLTherefore the volume of water that needs to be added is 120mL (minus the original volume).
20.2 g of CuCl2 = .1502 mol CuCl2 M=mol/L M=.1502 mol/L
Initially, the mass of H2SO4 required to prepare 5.8 liters of 1.5 molar solution should be calculated. Number of moles present in 5.8 L of 1.5 molar solution = 1.5 mol L-1 x 5.8 L= 8.7 molMolar mass of H2SO4 = 98 g mol-1Therefore, mass of H2SO4 in the above solution = 8.7 mol x 98 g mol-1= 852.6 gMass of H2SO4 in the original solution per litre = 1.531 g x 32/100= 0.48992 gVolume of sulphuric acid required to prepare 1.5 molar solution = 852.6 g/0.48992 g = 1740.3 L
The molarity is 2 mol/L.
0.045 mol L 0.5. Mol.
202.44
For starters, you know that 0.05000-mol L − 1 solution of copper(II) sulfate contains 0.05000 moles of copper(II) sulfate, the solute, for every 1 L = 10 3 mL of the solution.
Molarity equals mole per liter M = mol/L So solve for moles by multiplying liters to the other side of the equation and you get: mol=ML Plug in your numbers mol=0.250M*2.00L mol=0.5 or 19,99855 grams = aprox. 20 grams
Applying the equation for a dilution (c1.V1 = c2.V2) gives4.0(mol/L)*V1(L) = 2.5(mol/L)*4.5(L) so V1 = 2.5*4.5/4.0 = 2.813 L = 2.8 litres
4.25 grams. .050 M = .050 mol/1 L 5.0 L x .050 mol/L (cancel out L to get mol as a unit)= .25 mol Atomic mass of Ammonia (NH3)= 17 g/mol .25 mol x 17 g/mol (cancel out mol to get g as a unit)= 4.25 g
Wouter Mol was born on 1982-04-17.
Multiply the molarity (M, which is in mol/L) with the volume (in L) to get the number of moles needed. Then multiply the result with the molar mass. If you look at the units they will cancel to give an answer in grams. (mol/L)*(L)=mol, (mol)*(g/mol)=g So for the numerical answer you get (0.0552 mol/L)*(0.750 L)*(119.00 g/mol)= 4.93 g KBr
C1V1 = C2V24 x .04 = 1 x V2V2 = (4 x .04)/1= 160mLTherefore the volume of water that needs to be added is 120mL (minus the original volume).
2.5 0.05 L (50 mL) * 15 Mol/L= 300 Mol/L * X litres (0.05 L * 15 Mol/L) / 300 Mol/L = 0.0025 L or 2.5 mL
0.5 Moles If you have a 0.25 M solution, you have 0.25 mol/dm3, or 0.25 moles in 1 L (0.25 mol/L) If you have 2 L of solution, you have 2 L x 0.25 mol/L = 0.5 mol The L's cancel out, and you're left with moles.
You will mix NH4OH with water. To get a specific concentration you will need to calculate the number of moles required and covert this to a mass. Use the molar mass of NH4OH. eg. 100 mL of 0.5 mol/L NH4OH -> 35.06 g/mol x 0.5 mol/L x0.100 L Notice the units cancel to g. Obtain this amount using a balance and add water to 100mL.
This molarity is 3 mol/L.