Balanced Equation.
NaOH + HNO3 >> NaNO3 + H2O
Now, Molarity = moles of solute/liters of solution
0.800M HNO3 + mol/2.50L
mol of HNO3 = 2
2mol HNO3 (1mol NaOH/1molHNO3 )(39.998g NaOH/1mol NaOH )
= 79.996 grams
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
----------------------------
First write the BALANCED reaction equation.
NaOH + HNO3 = NaNO3 + H2O
The molar ratios are 1:1::1:1
So be equivalence
it is 0.2:0.2:: 0.2 :0.2
So you require 0.2 moles NaOH
The reaction to completion will produce 0.2 moles (NaNO3) and 0.2 moles water.
NaOH + HNO3 --> H2O + NaNO3
(0.20 mol HNO3) x (1 mol NaOH) / (1 mol HNO3) = 0.20 mol NaOH
0,2 mol of NaOH is sufficient
0.20mol
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.
short answer: nolong answer: if you have to ask, you should not be using this stuff
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 symbol for Sodium Hydroxide is NaoH
20 moles of NaOH needed to neutralize 20 moles of nitric acid
98g
262 - 266
262 - 266
97.8 - 98.2 98 worked for me
Hydroxide compounds such as sodium hydroxide (NaOH) are bases. Bases do not neutralize other bases. Acids neutralize bases.
The best way to neutralize nitric acid is with sodium bicarbonate (baking soda).
sodium nitrate + water
Coefficients of nitric acid Sodium hydroxide sodium nitrate+water
sodium nitrate
No, adding solid sodium hydroxide to neutralize hydrochloric acid (HCl) would not cause sodium chloride to redissolve. The reaction between sodium hydroxide and hydrochloric acid forms water and sodium chloride, which remains in its dissolved form. The addition of solid sodium hydroxide would simply further neutralize the acid and increase the concentration of the resulting sodium chloride solution.
Acids: hydrochloric acid, sulphuric acid, nitric acid Bases: sodium hydroxide, potassium hydroxide, sodium methoxide