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HNO3 or Nitric acid seldom used to prepare standard acid solutions because it is not suitable to use as a primary standard because it always contains a little nitrous acid, HNO2, which has a destructive action on many acid-base indicators.
Syrhene Descalso
Wiki User
∙ 11y agoIt is because of their oxidizing properties.
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Why is nitric acid not often used as a standard solution for neutralization titrations?
The usual primary standard for acid-base titration is sulfuric acid. Nitric acid tends to lose NO2 by volatilization and HCl is also more volatile.
Comparison between dilute solution of nitric acid and a concentrated nitric acid?
The diluted solution has a slight hint of red as the other is just clear
How Cerium can be separated from the solution of lanthenides?
by leaching the solution with nitric acid
Which metal doesn't react with nitric acid?
Nitric Acid cannot react with Gold alone. The only solution that can dissolve Gold is Aqua Regia; a combination of Nitric Acid and Hydrochloric Acid.
What volume of concentrated nitric acid 15.0 is required to make 300mL of a 2.5 M nitric acid solution?
12.5
Why is nitric acid not often used as a standard solution for neutralization titrations?
The usual primary standard for acid-base titration is sulfuric acid. Nitric acid tends to lose NO2 by volatilization and HCl is also more volatile.
Comparison between dilute solution of nitric acid and a concentrated nitric acid?
The diluted solution has a slight hint of red as the other is just clear
How Cerium can be separated from the solution of lanthenides?
by leaching the solution with nitric acid
Which metal doesn't react with nitric acid?
Nitric Acid cannot react with Gold alone. The only solution that can dissolve Gold is Aqua Regia; a combination of Nitric Acid and Hydrochloric Acid.
What volume of concentrated nitric acid 15.0 is required to make 300mL of a 2.5 M nitric acid solution?
12.5
Is nitric acid a dilute acid?
Nitric acid can be dilute or concentrated. This is simply a matter of how much of it you have in a given amount of a solution, which is variable.
A nitric acid solution is neutralized using sodium hydroxide how many grams of sodium hydroxide are needed to neutralize 3.50L of 0.700 M nitric acid solution?
98g
A nitric acid solution is neutralized using sodium hydroxide how many grams of sodium hydroxide are needed to neutralize 5.50 L of 1.200M nitric acid solution?
262 - 266
What solution will dissolves the metal gold?
Aqua regia (mixture of concentrated nitric acid and hydrochloric acid). However, nitric acid and hydrochloric acid by themselves don't dissolve gold.
A nitric acid solution is neutralized using sodium hydroxide How many grams of sodium hydroxide are needed to neutralize 5.50 L of 1.200 M nitric acid solution?
262 - 266
How do you prepare 5 percent nitric acid solution from 55 percent nitric acid?
To solve this problem, we basically have 2 equations and 2 unknowns. The unknowns are the (volume of water) & the (volume of 70 wt%) nitric acid to add. * This problem will assume that you are interested in making 1 L (or 1000 mL) of 5 wt% nitric acid solution. Equation 1: (volume of water) + (volume of 70 wt% nitric acid) = 1000 mL Equation 2: mass of nitric acid / [mass of water + mass of 70 wt% nitric acid solution] = 0.05 (0.05 is 5 wt%) * Remember that mass = density * volume * Remember that 70 wt% nitric acid solution mean that for 100 grams (gm) of this acid, then there's 70 grams of HNO3 * Remember that density of 70 wt% nitric acid solution is 1.413 gm/cm^3 * Remember that density of water is 1 gm/cm^3 Equation 2 is now re-written as: [(density of 70 wt% nitric acid soln)*(volume of 70 wt% nitric acid)*0.70] / [(volume water)*(1gm*cm^3) + (volume of 70 wt% nitric acid)*(1.413gm/cm^3)] = 0.05 Solving for the 2 equations gives answer to the 2 unknowns: Answer: To make 1000 mL of 5 wt% nitric acid solution, add 1) 51.63 mL of 70 wt% nitric acid solution 2) 948.37 mL of water
What are concentration of solution?
Examples: - concentrated solution of sulfuric acid - concentrated solution of nitric acid - concentrated solution of ethanol - concentrated solution of sugar (syrup) - concentrated solution of table salt
