Molarity = moles of solute/Liters of solution
0.343 M NaOH = moles NaOH.2.5 Liters
= 0.8575 moles NaOH (39.998 grams/1 mole NaOH)
= 34 grams of NaOH
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Any acid can be used to neutralize a base such as sodium hydroxide. If you have a concentrated solution of sodium hydroxide, you could neutralize it most efficiently with a strong acid such as hydrochloric acid. You can also neutralize it with Coca Cola, or vinegar, or many other acidic chemicals, but it would require a larger amount than if you used hydrochloric acid.
NaOH + HCL --> NaCl + H20 The basic equation is as follows: NaOH(aq) + HCl(aq) -----------> NaCl(aq) + H20(l) sodium hydroxide + hydrochloric acid ----> Sodium chloride + water. The molecules themselves dissociate in an equilibrium and so the ionic equation is: H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) ---------> Na+(aq) + Cl-(aq) + H2O(l). hope that helps
When just enough strong acid (e.g. HCl) is used to neutralize a strong base (NaOH), the pH should be neutral (pH = 7.0).
The largest volume of 0.100M sodium hydroxide solution would be needed to neutralize a strong acid with a low molarity. This is because a lower molarity acid would require more moles of sodium hydroxide to neutralize it, resulting in a higher volume of the solution being needed.
Any base or alkali. However, carbonates also neutralise acids. So using sodium carbonate, or calcium carbonate , both very common substances. Na2CO3 + 2HNO3 = 2NaNO3 + H2O + CO2 or CaCO3 + 2HNO3 = Ca(NO3)2 + H2O + CO2
The balanced chemical equation for the neutralization between sodium hydroxide (NaOH) and nitric acid (HNO3) is 1 mol of NaOH reacts with 1 mol of HNO3. Therefore, 20 moles of nitric acid would require 20 moles of sodium hydroxide to neutralize it.
98g
262 - 266
262 - 266
First, calculate the number of moles of nitric acid present in 3.50 L of 0.700 M solution. Since nitric acid is a diprotic acid, the mole ratio with sodium hydroxide is 1:2. Then, use the mole ratio to determine the number of moles of sodium hydroxide needed to neutralize the nitric acid. Finally, convert the moles of sodium hydroxide to grams using its molar mass.
To safely neutralize concentrated nitric acid, you can slowly add a base like sodium bicarbonate or sodium hydroxide while wearing protective gear and ensuring good ventilation. This will help to neutralize the acid and reduce its corrosive properties.
The salt formed when sodium hydroxide is added to nitric acid is sodium nitrate (NaNO3).
The balanced chemical equation for the reaction between nitric acid and sodium hydroxide is: HNO3 + NaOH -> NaNO3 + H2O. Therefore, the coefficient for nitric acid is 1, for sodium hydroxide is 1, for sodium nitrate is 1, and for water is 1.
To neutralize the nitric acid, you need a 1:1 mole ratio of sodium hydroxide to nitric acid. First, calculate the moles of nitric acid in the solution using the formula Molarity = moles/volume. Then, use the mole ratio to find the moles of sodium hydroxide needed. Finally, convert this to grams using the molar mass of sodium hydroxide.
sodium nitrate + water
The best way to neutralize nitric acid is with sodium bicarbonate (baking soda).
Sodium hydroxide is an alkali. It is a strong base that dissociates in water to form hydroxide ions, which can accept protons and neutralize acids.