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If 6.73g of Na2CO3 is dissolved in enough water to make 250ml of solution what is the molarity of the sodium carbonate what are the molar concentrations of the Na plus and CO32- ions?
To find the molarity of the Na2CO3 solution, first convert grams to moles using the molar mass of Na2CO3 (105.99 g/mol). Calculate the number of moles in 6.73g, then divide by the volume in liters (0.25 L) to get the molarity. Since each Na2CO3 molecule gives 2 Na+ ions and 1 CO32- ion when dissolved, the molar concentration of Na+ ions would be twice the molarity calculated, and the molar concentration of CO32- ions would be equal to the molarity.
What is the molarity of 20.2 g of potassium nitrate in enough water to make 250.0 mL of solution?
To find the molarity, first calculate the number of moles of potassium nitrate using its molar mass (101.1 g/mol). This comes out to 0.2 moles. Then, divide the moles by the volume of the solution in liters (0.250 L) to get the molarity, which is 0.8 M.
What is the molarity of the solution where 0.5 g of NaCl is dissolved to make 0.05 L of solution?
Given: 0.5 g NaCl; 0.05 L of solution.1) Find the molar mass of NaCl.(22.99) + (35.45) = 58.44 g/mol of NaCl2) Convert grams of NaCl to moles of NaCl.(0.5 g NaCl) X (1 mol NaCl / 58.44 g NaCl) = 0.00855578 mol NaCl3) Use the molarity equation, M = mol / L, to solve for molarity (M).(0.00855578 mol NaCl / 0.05 L) = 0.17 M
What is the molarity of the solution formed by mixing 0.20 mol of sodium hydroxide with enough water to make 150 ml of solution?
To calculate the molarity of the solution, first convert the volume to liters (150 mL = 0.150 L). Then, divide the moles of solute (0.20 mol NaOH) by the volume of solution in liters to get the molarity. Molarity = 0.20 mol / 0.150 L = 1.33 M.
What is the molarity of sodium sulphate in a solution prepared by dissolving 15.5g in enough water to make 35ml of solution?
Molarity = moles of solute/volume of solution Find moles NaCl 55 grams NaCl (1mol NaCl/58.44 grams) = 0.941 moles NaCl Molarity = 0.941 moles NaCl/35 Liters = 0.027 Molarity NaCl ( sounds reasonable as 55 grams is not much in 35 Liters of water, which would be about 17.5 2 liter sodas )
Calculate the molar it’s oh a solution that contains 15.7 of CaCO3 dissolved in enough water to make 275mL of solution?
0.570 M (note the capital M, this is molarity.)
184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500.0 mL of solution?
The molarity is 0.001255. Should you really be asking an AP Chem question on Wiki Answers, anyways?
2.431 g of h2c2o4 x 2h2o was obtained and dissolved in enough dI water to form 250.0 ml of solution what is the concentration of the resulting of h2c2o4 solution?
Molarity (concentration ) = moles of solute/Liters of solution 250.0 ml = 0.250 liters 2.431 grams H2C2O4 * 2H2O ( 1mole cpd/ 126.068 grams) = 0.01928 moles H2C2O4 * 2H2O Molarity = 0.01928 moles cpd/0.250 liters = 0.07712 Molarity
What is the molarity of a solution made by dissolving 23.4g of sodium sulphate in enough water to make up a 125ml solution?
To find the molarity, first calculate the number of moles of sodium sulphate using its molar mass. Sodium sulphate's molar mass is 142.04 g/mol. Next, divide the number of moles by the volume in liters (125 ml = 0.125 L) to get the molarity. This will give you the molarity of the sodium sulphate solution.
What is the amount of solute dissolved in a given amount of solvent?
This is known as the concentration or more technically the molarity or molality of the solution.
What is the molarity of a solution made by dissolving 3.09 moles of Nacl in 1.50 L of solution?
what is the molarity of a solution prepared by dissolving 36.0g of NaOH in enough water to make 1.50 liter of solution?
To 225 mL of a 0.80M solution of KI a student adds enough water to make 1.0 L of a more dilute KI solution What is the molarity of the new solution?
0.18M
18.6 grams of a solute with molecular mass of 8490 grams are dissolved in enough water to make 1.00 dm3 of solution at 25 Celsius what is the osmotic pressure of the solution?
To calculate the osmotic pressure of the solution, you can use the formula: π = iMRT, where i is the van't Hoff factor (number of particles into which the solute dissociates), M is the molarity of the solution, R is the ideal gas constant, and T is the temperature in Kelvin. First, find the molarity (M) by dividing the mass of the solute by its molecular mass and the volume of the solution in liters. Then, plug in the values and calculate the osmotic pressure.
How do you determine the molarity of a solution containing 18.2g C6H12O6and enough water to reach 6.3L?
Moles of solute ---------------- Liters of solution So, convert your grams to moles by dividing by the molar mass (add together the atomic masses of the solution) and then that will give you your moles. Divide that number by your 6.3 Liters. That number is your molarity.
What is the molarity of a solution formed by mixing 20.0 g sulfuric acid with enough water to make 500.0 mL of solution?
To find the molarity, start by converting grams of sulfuric acid to moles. the molar mass of sulfuric acid (H2SO4) is 98.08 g/mol. Divide the moles by the volume in liters (500.0 mL = 0.5 L) to get the molarity. Molarity = moles/volume (L).
If 6.73g of Na2CO3 is dissolved in enough water to make 250ml of solution what is the molarity of the sodium carbonate what are the molar concentrations of the Na plus and CO32- ions?
To find the molarity of the Na2CO3 solution, first convert grams to moles using the molar mass of Na2CO3 (105.99 g/mol). Calculate the number of moles in 6.73g, then divide by the volume in liters (0.25 L) to get the molarity. Since each Na2CO3 molecule gives 2 Na+ ions and 1 CO32- ion when dissolved, the molar concentration of Na+ ions would be twice the molarity calculated, and the molar concentration of CO32- ions would be equal to the molarity.
18.6 grams of a solute with molecular mass of 8940 grams are dissolved in enough water to make 1.00 dm of solution at 25 àC What is the osmotic pressure of the solution?
Using the formula for osmotic pressure π = iMRT, where i is the van't Hoff factor, M is the molarity in mol/L, R is the gas constant, and T is the temperature in Kelvin, we can calculate the osmotic pressure. First, determine the number of moles of solute in the solution using the given mass and molecular mass. Then calculate the molarity of the solution. Finally, plug in the values and solve for the osmotic pressure.
