What is the molarity of the solution?
Let’s learn what is the molarity of the solution. The most accurate or helpful solution is served by Yahoo! Answers.
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What would be the molarity of a solution in which 5.6 mole of KOH is dissolved in enough water to make 0.43 L of solution? What would be the molarity of a solution in which 0.69 mole of NaCl is dissolved in enough water to make 3.4 L of solution?
Answer:
Molarity = (moles of solute) ÷ (liters of solution) What would be the molarity of a solution...
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Other solutions
An aqueous solution is 6.00% methanol by mass( CH3OH) by mass with density 0.988mg/L.What is the molarity. I got this far: Assuming the solution is 1000ml m=d*v so 0.988*1000=988g Mass of solution=988g and i know molarity= amount of substance/ volume...
Answer:
Start by taking a 1.0L solution Mass of this solution is: 988g - from the density The methanol is 6...
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if dissolved 6.96mg of arginine (MW=174) in 100 ml of solution, what is the molarity of solution? molarity is something i can never get.. please helpp
Answer:
m=0.00696g n=m/M=0.00696/174=4*10^-5 mol then 100mL=0.1L so Molarity =n/V=4*10^-5/0.1=4*10^-4mol/L
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Answer:
moles = conc x volume 0.355M x 0.0282L= 0.01 moles of H2SO4. Remember sulphuric acid is diprotic so...
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Answer:
HCl + NaOH --> NaCl + H2O (reaction of Titration) Number of Moles of NaOH = 0.1051*37.22 ml / 10...
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Answer:
Morality = Moles of solute/ Liters of solution The solute in the problem is glucose which is C6H12O...
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Answer:
Molarity is moles/per liter so: 2.8 moles * 1000/300ml will be your answer.= 28/3 Molarity
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if 2 moles of NaCl dissolve in water to make 500.0mL solution, what is the molarity of the solution? 1) 2.5M 2) 4.0M 3) 3.1M 4) 1.0M
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what is the molarity of an NaI solution that contains 6.00g of NaI in 20.0 ml of solution
Answer:
Molar mass NaI = 149.89 g/mol 6.00g = 6.00/149.89 = 0.0400 mol NaI Dissolved in 20mL solution = 0.0...
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What is the molarity of a solution containing 9.0 moles of solute in 500.0 mL of solution? Don't forget the unit. Please help! I have no idea how to solve this :(
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