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A 60.0 g sample of Na-OH is dissolved in water and the solution is diluted to give a final volume of 3.00 L what is the molarity of the final solution?
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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?
What is the molarity of a solution if 48.0 mL of a 0.220 M solution is required to neutralize a 25.0-mL sample of the solution?
.430
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
WHY pH increases of strong acid when diluted?
When the acid is is diluted; its pH has a chance increase above seven and nake the sample;solution; Etc acidic.
If a 25 g sample of sugar was dissolved in 50 g of water The concentration of the solution is?
33% by mass
A sample of 76g of NaCl is dissolved to make 1L of solution. what is the molarity of the solution?
1.3g
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?
What is the molarity of a solution if 48.0 mL of a 0.220 M solution is required to neutralize a 25.0-mL sample of the solution?
.430
What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below?
What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below?
If 57.0 mL of BaCl2 solution is needed to precipitate all the sulfate ion in a 742 mg sample of Na2SO4 what is the molarity of the solution?
22
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
WHY pH increases of strong acid when diluted?
When the acid is is diluted; its pH has a chance increase above seven and nake the sample;solution; Etc acidic.
A 20.0 mL sample of CuSO4 was evaporated to dryness leaving 0.967g of residue What was the molarity of the original solution?
Molarity = moles of solute(CuSO4)/volume of solution(Liters) 0.967 grams CuSO4 (1 mole CuSO4/159.62 grams) = 0.00606 moles CuSO4 Molarity = 0.00606 moles/0.020 liters = 0.303 Molarity
If the filtrate is a solution how do you obtain a dry sample of the salt dissolved?
Boil the solution and the solvent will get evaporated and you will get the dry salt
A 2.14g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution the solution pH is 11.32 what is the KB for the hypoiodite ion?
A 2.14-g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution pH is 11.32. What is Kb for the hypoiodite ion?
If 2.14 L sample of hydrogen chloride HCL gas at 2.61 ATM and 28 C is completely dissolved in 668 ml of water to form hydrochloric acid solution Calculate the molarity of the acid solution?
PV = nRT --> n = PV/RT n = moles of HCl = (2.61 atm)(2.14 L)/(0.0821)(273+28) = 0.226 moles Molarity = 0.226 moles/0.668L = 0.338 M
Why sample need to be diluted?
why the sample need dilution
