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What volume in mL of a 1.06 M NaOH solution is required to neutralize 11 g of HCl?
Wiki User
∙ 13y ago
Balanced equation.
NaOH + HCl -> NaCl + H2O
all one to one. find moles HCl.
11 grams HCl (1 mole HCl/36.458 grams ) = 0.3017 moles HCl
Moles HCl same as moles NaOH
Molarity = moles of solute/Liters of solution
1.06 M NaOH = 0.3017 moles NaOH/liters of solution
= 0.2846 Liters
this is equal to..... 285 milliliters of NaOH needed
Wiki User
∙ 13y ago
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What volume (in liters) of a 1.9 M NaOH solution would neutralize 7.2 moles of H2SO4 (diprotic)?
The answer is 7,66 L.
How many grams of solid NaOH are needed to prepare 500mL NaOH solution with a concentration of 0.4M?
molarity equals moles of solute /volume of solution in litres . moles of NaOH equals 5g/40g = 0.125 and volume of solution will be volume of water + volume of NaOH = 0.5 litre+0.002 l which is nearly 0.5 litre . (volume of NaOH is calculated by its density) so molarity = 0.125mol/0.5litre = 0.25 M
What amount of NaOH is required to prepare 1N NaOH solution and why only that amount is used?
40 grams, this is the 1M NaOH standard laboratory solution.
What is the purpose of adding NaOH to the mixture before taking the polarimeter reading?
It is to neutralize the solution and to stop the hydrolysis.
What volum of 0.502 m naoh solution would be required to neutralize 27.2 ml of 0.491 m hno solution?
The molar weight of NaOH is 39.9971 g/mol. .15g is 3.75 millimoles. The reaction of H2SO4 and NaOH is H2SO4 + 2 NaOH --> Na2SO4 + 2 H2O. So the molar ratio of H2SO4 to NaOH is 1:2. So it takes 1.825 millimoles of H2SO4. Volume = molars/concentration. Then it takes 14.96 mL of H2SO4.
A solution of malonic acid h2c3h2o4 was standardized by titration with 0.1000 M Naoh solution if 20.76 ml of the naoh solution were required to neutralize completely 13.15 ml of malonic acid solution?
.0899M
What volume (in liters) of a 1.9 M NaOH solution would neutralize 7.2 moles of H2SO4 (diprotic)?
The answer is 7,66 L.
How many grams of solid NaOH are needed to prepare 500mL NaOH solution with a concentration of 0.4M?
molarity equals moles of solute /volume of solution in litres . moles of NaOH equals 5g/40g = 0.125 and volume of solution will be volume of water + volume of NaOH = 0.5 litre+0.002 l which is nearly 0.5 litre . (volume of NaOH is calculated by its density) so molarity = 0.125mol/0.5litre = 0.25 M
What volume of a 0.187 M sodium hydroxide solution is required to neutralize 11.9 mL of a 0.144 M hydrobromic acid solution?
NaOH + HBr ==> NaBr + H2O They react in a 1:1 ratio. Thus, (x ml)(0.187 M) = (11.9 ml)(0.144 M) and x = 9.16 mls
What amount of NaOH is required to prepare 1N NaOH solution and why only that amount is used?
40 grams, this is the 1M NaOH standard laboratory solution.
What is the purpose of adding NaOH to the mixture before taking the polarimeter reading?
It is to neutralize the solution and to stop the hydrolysis.
What volum of 0.502 m naoh solution would be required to neutralize 27.2 ml of 0.491 m hno solution?
The molar weight of NaOH is 39.9971 g/mol. .15g is 3.75 millimoles. The reaction of H2SO4 and NaOH is H2SO4 + 2 NaOH --> Na2SO4 + 2 H2O. So the molar ratio of H2SO4 to NaOH is 1:2. So it takes 1.825 millimoles of H2SO4. Volume = molars/concentration. Then it takes 14.96 mL of H2SO4.
A nitric acid solution is neutralized using sodium hydroxide How many grams of sodium hydroxide are needed to neutralize 2.50 L of 0.800 M nitric acid solution?
Make sure that the equation is balanced. NaOH + HNO3 > > NaNO3 + H2O ( all one to one ) 15.0 grams NaOH (1mol NaOH=39.998g) (1mol HNO3/1mol NaOH) = 0.375 moles of HNO3 Molarity = mols solute/volume solution 2.00M HNO3 = 0.375 mols/X volume = 0.188 Liters or, 188 milliliters.
What volume of 2.5 M NaOH solution is required to prepare 2.0 liters of a 0.75M NaOH?
Simple equality will do here as you have three things and require a fourth. (X L)(2.5 M NaOH) = (2.0 L)(0.75 M NaOH) 2.5X = 1.5 X = 0.60 Liters needed ================
How many ml of 250 M NaOH are required to neutralize 30.4 ml of 152 M HCl?
M1V1=M2V2... By plugging in, you get 18.48 mL of NaOH
How much NaOH is in 3.8 L of a 0.53 M NaOH solution?
Molarity = moles of solute/volume of solution 0.53 M NaOH = moles NaOH/3.8 Liters = 2.014 moles, or about 80 grams
What happened if some solution splashes out during the titration of NaOH?
If some solution splashes out during the titration of NaOH, the volume at the end point will be wrong.
