It depends on the concentration of the solution.
If you know the concentration(molarity) then use the equation.
moles = [conc] x vol(mL) / 1000
NB The '1000' isusedto convert the concentration units of moles per litre (molL^-1) to mL.
Start with CaCl2. 250ml of 0.20M solution will give (0.2/1000)*250 moles = 0.05 moles. However, CaCl2--> Ca2+ + 2Cl- (1:2 reaction) so 0.05moles of CaCl2 will give 2* 0.05 moles cl ions =0.1moles. KCl will give (0.4/1000)* 250 moles =0.1 moles Since KCl--> K+ + Cl- (1:1 reaction) so 0.1 moles KCl will give 0.1 moles Cl ions. Add the 2 together so 0.1moles + 0.1 moles = 0.2 moles in total.
Molarity is moles of solute / liters of solvent. Plugging in the data: 0.236M = x / 0.250L; x = (0.236M)(0.250L) = 0.0590 moles of CaCl2. The molecular weight of CaCl2 is 40.1 + 2(35.5) = 111.1 g / mole. The mass of CaCl2 = (MW)(moles) = (111.1g/mole)(0.0590moles) = 6.55g
C7H5N3O6 Molarity = moles of solute/Liters of solution (250 ml = 0.25 Liters ) 0.100 M C7H5N3O6 = X moles/0.25 L = 0.025 moles -------------------------now, 0.025 moles C7H5N3O6 (227.14 grams/1 mole C7H5N3O6) = 5.68 grams TNT ====================a good firecracker!
To prepare a 2 M solution of KOH, you would need to calculate the moles of KOH required first. Then use the formula mass of KOH (56 g/mol) to convert moles to grams. First, calculate the moles needed: 2 moles/L * 0.25 L = 0.5 moles. Then, convert moles to grams: 0.5 moles * 56 g/mole = 28 grams of KOH needed.
To find the final concentration, we calculate the moles of KOH initially present in the 45.0 ml solution, then add the moles from the additional 250 ml of water. We then divide the total moles by the final volume (45.0 ml + 250 ml) to get the concentration. The concentration of the final solution would be less than 4.2 M KOH due to dilution when water is added.
Start with CaCl2. 250ml of 0.20M solution will give (0.2/1000)*250 moles = 0.05 moles. However, CaCl2--> Ca2+ + 2Cl- (1:2 reaction) so 0.05moles of CaCl2 will give 2* 0.05 moles cl ions =0.1moles. KCl will give (0.4/1000)* 250 moles =0.1 moles Since KCl--> K+ + Cl- (1:1 reaction) so 0.1 moles KCl will give 0.1 moles Cl ions. Add the 2 together so 0.1moles + 0.1 moles = 0.2 moles in total.
0.230 L X 0.276M CaCl2 = 0.0635 moles CaCl2 present in solution.Moles before dilution = moles after dilution0.0635 moles/V = 1.10 M CaCl2.V = 0.0577 L left in solution.0.230 L (original) - 0.0577 L (left over) = 0.172 L (evaporated)0.172 L = 172 mL
Molarity is moles of solute / liters of solvent. Plugging in the data: 0.236M = x / 0.250L; x = (0.236M)(0.250L) = 0.0590 moles of CaCl2. The molecular weight of CaCl2 is 40.1 + 2(35.5) = 111.1 g / mole. The mass of CaCl2 = (MW)(moles) = (111.1g/mole)(0.0590moles) = 6.55g
To find the final concentration of Cl- ions, first calculate the moles of Cl- ions from each solution. Then add the moles of Cl- ions from both solutions and divide by the total volume of the mixed solution (500 ml) to get the final concentration. Using the formula C1V1 = C2V2 where C represents concentration and V represents volume, you can determine the moles of Cl- ions from each solution.
To calculate the number of moles in a solution, use the formula: moles = Molarity x Volume (in liters). First, convert the volume from milliliters to liters by dividing by 1000 (250 mL = 0.25 L). Then, plug the values into the formula: moles = 1.20 mol/L x 0.25 L = 0.30 moles of sodium chloride.
C7H5N3O6 Molarity = moles of solute/Liters of solution (250 ml = 0.25 Liters ) 0.100 M C7H5N3O6 = X moles/0.25 L = 0.025 moles -------------------------now, 0.025 moles C7H5N3O6 (227.14 grams/1 mole C7H5N3O6) = 5.68 grams TNT ====================a good firecracker!
Molarity of a solution is the number of moles of the solute divided by the volume of the solution (in liters). If 750 ml of 20M HCl is mixed with 250 ml of 60M HCl, we first find the total number of moles of HCl in our new solution. Using that same formula, M=moles/V, we cansee that moles=MV. In the first solution we have (20M)(0.750L) = 15 moles. In the second, (60M)(0.250L) = 15 moles, so we have a total of 30 moles in our new solution, which also has a volume of 750mL + 250mL = 1L. The molarity of the new solution is 30 moles/1L = 30M
250 g iron (III) oxide is equal to 1,565 moles.
The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters. In this case, there are 2 moles of sodium chloride in 250 cm^3, which is equivalent to 0.25 L. Therefore, the molarity of the solution is 8 M (2 moles / 0.25 L).
To prepare a 2 M solution of KOH, you would need to calculate the moles of KOH required first. Then use the formula mass of KOH (56 g/mol) to convert moles to grams. First, calculate the moles needed: 2 moles/L * 0.25 L = 0.5 moles. Then, convert moles to grams: 0.5 moles * 56 g/mole = 28 grams of KOH needed.
To find the final concentration, we calculate the moles of KOH initially present in the 45.0 ml solution, then add the moles from the additional 250 ml of water. We then divide the total moles by the final volume (45.0 ml + 250 ml) to get the concentration. The concentration of the final solution would be less than 4.2 M KOH due to dilution when water is added.
Molar mass of KCl = 39 g/mol (K) + 35.5 g/mol (Cl) = 74.5 g/mol. A 0.5 M solution is required (0.5 mol/L or 0.5 moles per litre). 0.5 moles of KCl is 0.5 mol x 74.5 g/mol = 37.25 g. Dissolving this 37.25 g of KCl in a litre of water would give a 0.5 M solution. If 1 L or 1000 mL of 0.5 M solution contains 0.5 moles then 1 mL of the same concentration solution would contain 0.5/1000 moles and 250 mL would contain 250 x 0.5/1000 moles = 0.125 moles. 0.125 moles of KCl is 0.125 mol x 74.5 g/mol = 9.31 g.