Simple equality.
(X L)(2.5 M HCl) = (1.5 L)(5.0 M NaOH)
2.5X = 7.5
X = 3.0 Liters needed
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This sounds like a typical neutralization reaction, so finding the moles of NAOH ( really OH-, but all one to one ) should suffice.
Molarity = moles of solute/liters of solution
or, for our purposes
moles of solute = liters of solution * Molarity
moles of NaOH = 1 liter * 5 M
= 5 moles NaOH
and if reaction is one to one
5 moles of H+ needed for complete neutralization
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Well, I'd have thought it would just be 5 moles, wouldn't it?
5HCl + 5NaOH > 5NaCl + 5H2O
or
HCl + NaOH > NaCl + H2O
If you are looking for the reaction to go to completion, then 0.005mol of HCl are required, because the reaction happens in a 1:1 stoichiometric ratio: HCl + NaOH --> NaCl + H2O.
This neutralization reaction is:
HCl + NaOH = NaCl + H2O
For 0,005 moles of sodium hydroxide the necessary amount of hydrogen chloride is also 0,005 moles.
30
One mole to react with ONE mole CH3COOH (ethaancarbonic acid) because it has only ONE proton (H+) to react with, the other 3 Hydrogen's are not proteolytic (=NON-acidic)
To neutralize HCl with NaOH, the mole ratio is 1:1. So, the moles of HCl are 0.200 M x 0.020 L = 0.004 moles. Since NaOH and HCl react in a 1:1 ratio, we need 0.004 moles of NaOH. Using the molarity formula, we find that we need 0.010 L or 10.00 mL of 0.400 M NaOH.
To calculate the number of moles of NaOH required to neutralize 50 mL of HCl, first convert 50 mL to liters. Next, use the molarity of NaOH (0.24 M) to determine the moles of NaOH required. Since HCl and NaOH react in a 1:1 ratio, the moles of NaOH will be equal to the moles of HCl.
The balanced chemical equation for the reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl) is 1 mol NaOH : 1 mol HCl. Calculate the amount of NaOH required by converting the given mass of HCl to moles using its molar mass, then use the mole ratio from the balanced equation to determine the moles of NaOH needed, and finally convert moles of NaOH to grams using its molar mass.
First, calculate the number of moles of HCl using the molar mass. Then, determine the number of moles of NaOH needed to neutralize the HCl based on the 1:1 stoichiometry of the reaction. Finally, use the molarity of NaOH to find the volume required using the formula Molarity = moles/volume.
The answer is 50 mL.
1337
You need 4 moles of NaOH to prepare 2 liters of a 2.0 M solution. This is calculated by multiplying the volume (2 L) by the molarity (2.0 mol/L). The result gives you the moles needed.
The mass of lead(II) nitrate required to react with 370 g NaOH is 1 531,9 g.
Molarity = moles of solute/Liters of solution 3.42 M NaOH = 1.3 moles NaOH/Liters NaOH Liters NaOH = 1.3 moles NaOH/3.42 M NaOH = 0.38 Liters
The molar mass of NaOH is 40 g/mol. Therefore, the mass of 3.42 moles of NaOH would be 40 g/mol x 3.42 mol = 136.8 grams.
First, calculate the number of moles of HCl using the molar mass. Then, determine the number of moles of NaOH needed to neutralize the HCl based on the 1:1 stoichiometry of the reaction. Finally, use the molarity of NaOH to find the volume required using the formula Molarity = moles/volume.
Since H2SO4 is a diprotic acid, it will require twice the amount of NaOH to neutralize it. Therefore, molarity of NaOH should also be 1 M. 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, to neutralize 1 mole of H2SO4, 2 moles of NaOH are required. To neutralize 1 mole of H2SO4 in 100 ml (0.1 L) of 1 M solution, you will need 0.1 moles of NaOH.
NaOH = 40 Mwt so 15/40 moles present. This requires 15/40 moles of HNO3 from the above equation. The HNO3 contains 2 moles in 1000 ml and so 1 mole in 500 ml and therefore 500 x 15/40 = 137.5 mls required
Na + 2H2O -----> H2 + NaOH If you have 2.5 moles water you need 1.25 mol elemental sodium
The limiting reagent in a reaction is the reactant that runs out first. For example, if you are reacting 10 moles of HCl and 5 moles of NaOH, you will get 5 moles of H20, 5 moles of NaCl, and 5 moles of HCl, because the remaining HCl had nothing to react with. Therefore, the NaOH is the limiting reagent.
To find the moles of HNO3 needed, we can use the formula: moles = Molarity x Volume (in liters). Substituting the values given, moles = 2.0 mol/L x 5.0 L = 10 moles of HNO3 needed to prepare a 2.0M solution in a 5.0 liter volume.