Calculate the concentration of nitric acid

Given: Density of nitric acid = 1.41 g/mol Percentage of Nitric acid = 69% 69% of nitric acid signifies 69g of nitric acid dissolved in 100g of solvent. Volume of nitric acid solution = [mass of solution]/ density of solution = 100/1.41 = 70.922 ml Number of moles of Nitric Acid = Mass of Nitric acid/ Molecular Mass of nitric acid = 69/63 = 1.095 moles Molarity, M o = 1092.5/70.92 = 15.404 M ≈ 15.4 M Therefore, concentration of nitric acid is 15.4 mole/L. 19 How many significant figures are present in the following? Rules for Determination of Significant Figures: [i] All non-zero digits are significant. For example: 146 cm has three significant figures. [ii] The zeros placed to the left of the first non-zero digit in the given physical quantity are not significant. For example: 0.56cm has two significant figures. [iii] The zeros placed to the right of the decimal point are significant. For example: 15,0cm has three significant figures. [iv] The zeros placed between two non-zero digits are significant. For example: 6.08cm has three significant figures. 24 Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: (i) Calculate the mass of ammonia produced if 2.00 × 10 3 g dinitrogen reacts with 1.00 × 10 3 g of dihydrogen. (ii) Will any of the two reactants remain unreacted? (iii) If yes, which one and what would be its mass? 34 A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen ...

I have quite a small quantity of concentrated nitric acid I had acquired about two years ago. This was given to me by a friend in a couple of Pyrex volumetric flasks with stopper and some in a borosilicate reagent bottles. The acid does have a whiskey brown color now. Is there any simple method or visual cue to identify what concentration the nitric acid could be with a simple test? I want to see if the acid is 70% nitric acid. If it's the higher concentration of 90%, then I want to dilute it to 70%. I have attached a picture of one of the bottles for reference to see the color below. $\begingroup$ @Mithoron I actually wanted some 70% acid. The reason I wanted to to know if there is any visual way or simple test to check concentration is because I haven’t really dealt with concentration nitric much. Only sulfuric and HCl. Become of the change in color from clear I was a bit confused if this is the 70% or 90%+ conc. $\endgroup$ It looks like you have about 40 mL of the solution. You could measure the density by using a small volumetric flask (10 or 25 mL), or even a graduated cylinder (which you could calibrate with water). Add your solution to the mark, weigh reasonably accurately, and you will have your answer (which I predict will lie between 70 and 90%). At 20C, the density of 70% acid is 1.41; the density of 90% acid is 1.48. The difference is large enough to determine easily, and if there is any deterioration, you should be able to determine the exact concentration fa...

The Complete Aqueous Nitric Acid Solutions Density-Concentration Calculator The Complete Aqueous Nitric Acid Solutions Density-Concentration Calculator This calculator calculates for concentration or density values that are between those given in the table below by a process called interpolation. Input a temperature and density within the range of the table to calculate for concentration or input concentration to calculate for density. The table below gives the density (kg/L) and the corresponding concentration (% weight) of Nitric Acid (HNO 3) solutions in water at different temperatures in degrees centigrade (°C). The table was taken from "Perry's Chemical Engineers' Handbook" by Robert H. Perry, Don Green, Sixth Edition. Click here for more Density-Concentration Calculators. Temperature Density Concentration °C kg/L % Weight Nitric Acid Solutions in Water Temperature in degrees Centigrade (°C) 0°C 5°C 10°C 15°C 20°C 25°C 30°C 40°C 50°C 60°C 80°C 100°C Concentration (% Weight) Density (kg/L) 1 1.0058 1.00572 1.00534 1.00464 1.00364 1.00241 1.0009 0.9973 0.9931 0.9882 0.9767 0.9632 2 1.0117 1.01149 1.01099 1.01018 1.00909 1.00778 1.0061 1.0025 0.9982 0.9932 0.9816 0.9681 3 1.0176 1.0173 1.01668 1.01576 1.01457 1.01318 1.0114 1.0077 1.0033 0.9982 0.9865 0.973 4 1.0236 1.02315 1.0224 1.02137 1.02008 1.01861 1.0168 1.0129 1.0084 1.0033 0.9915 0.9779 5 1.0296 1.02904 1.02816 1.02702 1.02563 1.02408 1.0222 1.0182 1.0136 1.0084 0.9965 0.9829 6 1.0357 1.03497 1.03397 1.03272 1.0...

Mass percent of nitric acid in the sample = 69 % [Given] Thus, 100 g of nitric acid contains 69 g of nitric acid by mass. Molar mass of nitric acid (HNO 3) = g mol –1 = 1 + 14 + 48 = 63 g mol –1 ∴ Number of moles in 69 g of HNO 3 Volume of 100g of nitric acid solution Concentration of nitric acid ∴Concentration of nitric acid = 15.44 mol/L

Learning Objectives • Give the names and formulas of some strong acids and bases. • Explain the pH scale, and convert pH and concentration of hydronium ions. • Evaluate solution pH and pOH of strong acids or bases. Acids and bases that are completely ionized when dissolved in water are called strong acids and strong bases There are only a few strong acids and bases, and everyone should know their names and properties. These acids are often used in industry and everyday life. The concentrations of acids and bases are often expressed in terms of pH, and as an educated person, you should have the skill to convert concentrations into pH and pOH. The pH is an indication of the hydrogen ion concentration, \(\ce\). Strong Acids Strong acids are acids that are completely or nearly 100% ionized in their solutions; Table \(\PageIndex\] Example \(\PageIndex) = 3.90851 \nonumber\] Strong Bases Strong bases are completely ionized in solution. Table \(\PageIndex \nonumber\] Example \(\PageIndex\] \[pH=14-pOH\] \[pH=14-3.6074\] \[pH=10.39\] Questions • What is the pH of a solution containing 0.01 M \(\ce\) Solutions • Answer 2 Hint... You do not need a calculator to evaluate \(-\log (0.01) = 2\) • Answer 12.64 Hint... \(\ce\) Consider... All others are weak acids

The concentration of an acid solution can be determined by titration with a strong base. First, calculate the number of moles of strong base required to reach the equivalence point of the titration. Then, using the mole ratio from the balanced neutralization equation, convert from moles of strong base to moles of acid. Finally, divide the number of moles of acid by the given volume of the acid solution to find the concentration. Created by Jay. When you divide both sides by 20 mL, the units cancel out so it does not matter what you choose. All that matters is that the unit you choose is the same throughout the equation. Dividing 27.4mL by 20mL is the same as dividing 0.0274L by 0.02L. You will get the same number and there will be no units! So, we can say that mL were used simply because the information was given in mL and it would have been unecessary to change. You have a base reacting with an acid. The question asks how much acid you need to react with base so that they neutralize each other (and form a salt with water, but no floating acids or bases). So, when are MV(basic)=MV(acidic). The greater volume that is made will not influence the equilibrium point because water is at pH 7 (neutral) so the ratio to total volume is irrelevant. Acids (using the Arrhenius definition) are chemicals which produce H+ ions, while bases are chemicals which produce OH- ions. So when barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl) enter a water solution they will dissociate, or s...

In chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. The standard formula is C = m/V, where C is the concentration, m is the mass of the solute dissolved, and V is the total volume of the solution. If you have a small concentration, find the answer in parts per million (ppm) to make it easier to follow. In a lab setting, you may be asked to find the Find the mass of the solute mixed in with the solvent. The solute is the substance that you’re mixing in to form your solution. If you’re given the mass of the solute in your problem, write it down and be sure to label it with the correct units. If you need to find the mass of the solute, then weigh it on a lab scale and record the measurement. X Research source • If the solute you’re using is a liquid, then you can also calculate the mass using the Record the total volume of the solution. The total volume of the solution is the amount of solvent plus the amount of solute added to it. If you’re finding the volume in a lab, mix the solution in a graduated cylinder or beaker and look at the measurement. Measure the volume from the curve at the top of the solution, or the meniscus, to get the most accurate reading. Record the volume of the solution. X Research source • If you aren’t measuring the volume yourself, you may need to convert the mass of the solute into volume using the density formula. • For example, if you’re finding th...

\( \newcommand \right ) \nonumber \] the required volume is 0.86 mL (there are only two significant figures in the concentration of the stock solution, 0.029 M). Dilution problems can be solved directly using the above equation, or, as you become more comfortable with the math, using the initial and final ratios like we did in this problem (remember, the numbers in the two ratios are “smaller/larger”). Exercise \(\PageIndex\) • A 1.50 mL aliquot of a 0.177 M solution of sulfuric acid (H 2SO 4) is diluted into 10.0 mL of distilled water, to give solution A. A 10.0 mL aliquot of A is then diluted into 50.0 mL of distilled water, to give solution B. Finally, 10.0 mL of B is diluted into 900.0 mL of distilled water to give solution C. Additional distilled water is then added to C to give a final volume of 1.0000 L. What is the final concentration of sulfuric acid in solution C? • A solution was prepared by mixing 250 mL of 0.547 M NaOH with 50.0 mL of 1.62 M NaOH and then diluting to a final volume of 1.50 L. What is the molarity of Na + in this solution? To what final volume should 75.00 mL of 0.889 M HCl(aq) be diluted to prepare 0.800 M HCl(aq)?