0
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of Solution
Volume of Solution required = 5.00L
We can say therefore that:
Number of Moles of NaOH needed to prepare the solution
= Concentration of NaOH * Volume of Solution required
Therefore:
Number of Moles of NaOH needed to prepare the solution
= 0.025M * 5.00L
= 0.125moles
From this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
What else can I help you with?
How many moles of agno3 are needed to prepare 0.50 l of a 4.0 m solution?
Molarity = moles of solute/liters of solution or, for our purposes moles of solute = liters of solution * Molarity moles of AgNO3 = 0,50 liters * 4.0 M = 2.0 moles of AgNO3 needed --------------------------------------
How many moles of NaOH are needed to prepare 2 liters of a 2.0 M solution?
4 moles or 160 g NaOH is required for one litre solution.
How many moles of NaOH needed to prepare 300 mL of a 0.2 m solution of NaOH?
To find the moles of NaOH needed, use the formula: moles = concentration (molarity) x volume (liters). First, convert 300 mL to liters (0.3 L). Then, calculate: moles = 0.2 mol/L x 0.3 L = 0.06 moles. Therefore, 0.06 moles of NaOH are needed to prepare 300 mL of a 0.2 M solution.
What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4?
To find the total number of moles needed, use the formula n = M x V, where n is the number of moles, M is the molarity, and V is the volume in liters. Thus, n = 2.0 mol/L x 5.0 L = 10 moles of H2SO4 are needed.
How many moles of NaOH are needed to prepare 2.00 L of a .250 M NaOH 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
How many moles of agno3 are needed to prepare 0.50 l of a 4.0 m solution?
Molarity = moles of solute/liters of solution or, for our purposes moles of solute = liters of solution * Molarity moles of AgNO3 = 0,50 liters * 4.0 M = 2.0 moles of AgNO3 needed --------------------------------------
How many moles of potassium hydroxide are required to prepare 300 mL of 0.250 M solution?
To calculate the moles of potassium hydroxide needed, use the formula: moles = molarity * volume (in liters). First, convert 300 mL to liters (0.3 L). Then, moles = 0.250 mol/L * 0.3 L = 0.075 moles of potassium hydroxide needed to prepare the solution.
How many moles of NaOH are needed to prepare 2 liters of a 2.0 M solution?
4 moles or 160 g NaOH is required for one litre solution.
How many moles of NaOH needed to prepare 300 mL of a 0.2 m solution of NaOH?
To find the moles of NaOH needed, use the formula: moles = concentration (molarity) x volume (liters). First, convert 300 mL to liters (0.3 L). Then, calculate: moles = 0.2 mol/L x 0.3 L = 0.06 moles. Therefore, 0.06 moles of NaOH are needed to prepare 300 mL of a 0.2 M solution.
How many moles of copper sulfate are needed to make 2.50 Liters of 0.125 moles solution?
0.125 Molar solution! Molarity = moles of solute/Liters of solution Algebraically manipulated, Moles of copper sulfate = 2.50 Liters * 0.125 M = 0.313 moles copper sulfate needed ===========================
What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4?
To find the total number of moles needed, use the formula n = M x V, where n is the number of moles, M is the molarity, and V is the volume in liters. Thus, n = 2.0 mol/L x 5.0 L = 10 moles of H2SO4 are needed.
How many moles of Fe3O4 are needed to prepare 4.74 moles of Fe2O3?
7.18
How many moles of NaOH are needed to prepare 2.00 L of a .250 M NaOH 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
How many liters are needed to make a 0.25 M solution with 0.50 moles moles of C12H22O11?
To find the volume of solution needed, you can use the formula: moles = Molarity × Volume. Rearranging the formula to solve for volume: Volume = Moles / Molarity. Plugging in the values, you get Volume = 0.50 moles / 0.25 M = 2 liters of solution needed.
How many grams of solid KOH is necessary to prepare 220.0 ml of 0.500 M KOH solution?
Molarity = moles of solute/Liters of solution ( 220.0 ml = 0.220 Liters ) 0.500 M KOH = moles KOH/0.220 Liters = 0.110 moles KOH (56.108 grams/1 mole KOH) = 6.17 grams solid KOH needed
How many grams of solute are needed to prepare 250.0ml of 0.125 M CuSO4?
To calculate the grams of solute needed to prepare a solution, you can use the formula: moles = Molarity x Volume (in liters). First, convert the volume to liters (250.0ml = 0.250L). Then, multiply the molarity (0.125 M) by the volume in liters to get the moles of CuSO4. Finally, multiply the moles by the molar mass of CuSO4 (159.61 g/mol) to get the grams needed. So, grams of CuSO4 needed = 0.125 mol/L x 0.250 L x 159.61 g/mol = 5.00 grams.
How many total moles of KNO3 must be dissolved in water to make 1.5 liters of a 2.0 M current?
To find the total moles of KNO3 needed, use the formula: moles = molarity x volume (in liters). So, moles = 2.0 mol/L x 1.5 L = 3.0 moles of KNO3. Therefore, 3.0 moles of KNO3 need to be dissolved in water to make 1.5 liters of a 2.0 M solution.
