it has a pH of 6 or very close to it
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.
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
It is able to (completely) donate its protons (H+) to water when in dilute solution (protolysis). This is what, according to Bronsted-Lowry, makes it a (strong) acid.HNO3 + H2O --> H3O+ + NO3-
Both are very strong acids in water.
The diluted solution has a slight hint of red as the other is just clear
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.
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
It is able to (completely) donate its protons (H+) to water when in dilute solution (protolysis). This is what, according to Bronsted-Lowry, makes it a (strong) acid.HNO3 + H2O --> H3O+ + NO3-
Copper reacts with nitric acid to produce copper (II) nitrate. In water, it forms a clear blue solution.
Both are very strong acids in water.
The diluted solution has a slight hint of red as the other is just clear
Nitric Acid + Sodium Hydroxide Solution = Fertilizer + 3x Water
by leaching the solution 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.
Yes, Nitrous is an unstable acid and only exists in water.
12.5
Vinegar: water+acetic acid Brandy: water+ethanol Diluted nitric acid: water+nitric acid