Nitric Acid Special Exercises synthesize all theoretical knowledge, illustrative examples and some types of multiple-choice exercises and essays on the topic of Nitric Acid (HNO3).
Through this document, it helps 11th graders to have more review materials, thereby strengthening their knowledge of Grade 11 Chemistry. At the same time, it helps teachers to have more teaching materials. In addition, you can refer to the exercises of Carboxylic Acid, exercises to calculate pH. Wish you all good study.
Nitric Acid Special Exercises
- A. Theoretical Summary of Nitric Acid
- II. Illustrated example of Nitric Acid
- III. Some types of exercises about Nitric Acid
- IV. Self-solution about Nitric Acid
- V. Nitric Acid Multiple Choice Exercises
A. Theoretical Summary of Nitric Acid
If a mixture of both metals and metal oxides reacts with HNO3 (and assuming NO gas is generated) then:
nHNO3 (po) = 4nNO + 2nO (in KL oxide)
II. Illustrated example of Nitric Acid
VD1. Completely dissolve mg of Cu powder in 800 g of HNO . solution3 get solution Y and 2.24 liters of NO gas (dktc). Y reacted sufficiently with 300 ml of 2 M NaOH solution precipitated R. After heating R to constant weight 20 g of solid was obtained.
a, Calculate the initial mass of Cu.
b. Calculate the mass of the substances in Y and the concentration % of the HNO . solution3used
nNO = 2.24/22.4 = 0.1 mol; nNaOH = 0.3.0.2 = 0.06 mol
When Y reacted with NaOH solution, a precipitate R containing only Cu(OH) was obtained.2.The solid obtained when calcined is CuO Þ nCuO = 20/80 = 0.25 mol = nCuO = 0.25 mol.
According to the law of conservation of elements:
nCu (original) = nCu (in CuO) = 0.25 mol mCu = 0.25.64 = 16 g
In X, n= = 0.25 mol m= 188.0.25 = 47 g
Cu → Cu2+ + 2e
0.25 mol 0.5 mol
0.3 mol 0.1 mol
Then show that the reaction of Cu and HNO3 must create SMALL4NO3.
ne (Give up) = Sni get it = 0.5 mol ni get it= 0.5 – 0.3 = 0.2 mol
III. Some types of exercises about Nitric Acid
Form 1: Metal reacts with HNO3
Acids react with Metals.
Lesson 1. Completely dissolve 1.2 grams of metal X in the HNO . solution3 The remainder obtained 0.224 liters of nitrogen gas only (unit ptc). Identify metal X?
Lesson 2. Dissolve 16.2 grams of trivalent metal in 5 liters of HNO . solution3 0.5 M (D = 1.25 g/ml). After the reaction finished, 2.8 liters of gas mixture X including NO, N . were obtained2 (0 .)oC, 2 atm). Mixing gas mixture X with enough oxygen after the reaction shows that the volume of gas is only 5/6 of the total volume of X and new oxygen is added.
a. Find used metal.
b. Calculate the % concentration of HNO . solution3after reaction.
Lesson 3. Completely dissolve 17.28 grams of Mg in the HNO . solution3 0.1M obtained solution A and 1,344 liters of gas mixture X including N2 and FEMALE2O (at 00C, 2 atm). Add an excess of KOH to solution A, and when heated, a gas is released. This gas acts just enough with 200 ml of H . solution2SO4 0.1 M. Calculate the volume of each gas in the mixture X?
Lesson 4. Let x mol of Fe react with a solution containing y mol HNO3 obtain only NO gas and solution B. What ions can exist in solution B? Explain the relationship between x and y so that in solution B there are ions.
Acid reacts with metal mixture.
Lesson 5. Determine the volume of HNO . solution3 What is the minimum 1M (dilution) required to completely dissolve a mixture of 0.15 mol Fe and 0.15 mol Cu (knowing the reaction that produces the only reducing agent is NO)?
Lesson 6. Completely dissolving 0.368 grams of Al and Zn mixtures requires 25 liters of HNO . solution3 pH = 3. After the reaction, solution A contains 3 salts (no gas is released).
a. Calculate the mass of each metal in the mixture.
b. Add an excess of SMALL solution to solution A3. Calculate the volume of the precipitate obtained.
Lesson 7. Mixture X consisting of Mg, Al, Zn with mass 8.6 grams is divided into 2 equal parts.
– Part 1: Burning completely in O2 7.5 g of the oxide mixture is obtained.
– Part 2: Dissolve in HNO . solution3 dense, hot, residual V liters (units) of NO . gas2 (single reduction product).
Lesson 8. Take mg of mixture X consisting of Cu and Fe (mass ratio 7:3) completely react with a solution containing 44.1 grams of HNO3; After the reaction, 0.75mg of solids and 5.6 liters of Y gas are left, including NO and NO .2 (dktc). Find m?
Type 2. Metal reacts with HNO . mixture3 and THEY2SO4
Lesson 1: Add 3.2 grams of Cu powder to 100 ml of a mixed solution of HNO3 0.8 M and H2SO4 0.2 M. After the reaction is complete, V liter of NO gas is produced (the only reduction product is achievable). Find the value of V?
Lesson 2: Completely dissolve mg of mixture X (Cu, Ag) in a solution containing HNO3 and THEY2SO4 obtained solution Y containing 7.06 grams of salt and gas mixture Z containing 0.05 mol NO2 and 0.01 mol SO2. What is the value of m?
Lesson 3: Let 12.9 grams of Al and Mg mixture react with 100 ml of mixed HNO . solution3 and THEY2SO4 0.1 mol of SO . gas was obtained2NO, FEMALE2O. How many grams of anhydrous salt did she get after the reaction?
Form 3: Prove the oxidizing property of NO3– Metals react with nitrate salts in an acidic environment
Lesson 1. For a quantity of Cu2S reacts completely with HNO . solution3 boil. The reaction to form solution Afirst and release A . gas2 Colorless, brown in air. Divide Afirst into two parts. Add BaCl . solution2 On part 1, a white precipitate A . was found3 insoluble in residual acids. Add SMALL residual solution3 in the second part and at the same time stirring the mixture, a solution of A . was obtained4 dark green in color.
a. Let’s determine AfirstA2A3A4what?
b. Write equations for the reactions that describe the above chemical processes.
Lesson 2. Add 19.2 g of Cu to 500 ml of NaNO . solution3 1M, then add 500 ml of 2M HCl to get a solution of A
a. Cu is completely melted? Calculate the volume of NO released at dtc.
b. Calculate the molar concentration of ions in solution A obtained after the reaction.
c. How many liters of 0.2 M NaOH solution must be added to precipitate all Cu .?2+contained in solution A.
Lesson 3. Dissolve 26.88 grams of copper metal powder in HNO . solution3 washy. After finishing the reaction, 4.48 liters of NO gas (dktc) was released and mg of insoluble matter remained. Slowly add V ml of 3.2 M HCl solution to dissolve just as much as mg of the insoluble substance, with NO gas released (only). Determine the value of V?
Lesson 4. Thoroughly stir the solution containing 13.6 grams of AgNO .3 with mg of Cu powder and then add to it 100 ml of H . solution2SO4 (diluted) and heated until the reaction is complete, 9.28 grams of metal powder, solution A and NO gas are obtained. The amount of NaOH required to completely react with the substances in solution A is 0.325 mol.
a. Calculate m and volume of NO gas collected at dtc.
b. Calculate the mass of the substances in solution A.
c. Calculate the molarity of H . solution2SO4use.
Lesson 5. For 5.8 grams of FeCO3 Sufficient effect with HNO . solution3 a mixture of two colorless gases browned in the presence of air and solution X. Add solution of H2SO4 If excess dilution is added to X, the resulting solution dissolves up to mg of Cu, given that the only reduction product is NO. What is the value of m?
Form 4. The problem of synthesizing nitric acid on metals
Lesson 1. Compare the volume of NO (only) gas released in the following 2 experiments (gases measured under the same conditions):
TN1: For 3.84 grams of Cu react with 80 ml of HNO . solution3 1.0 mol/liter.
TN2: For 3.84 grams of Cu react with 80 ml of solution containing HNO3 1.0 mol/liter and H2SO4 0.5 mol/liter.
Lesson 2. Heating x mol of Fe in air for some time yields 16.08 grams of a mixture of H consisting of 4 solids including Fe and its 3 oxides. Dissolve all the above mixture with HNO . solution3 Diluted, 672 ml of NO gas was obtained (according to the standard). Determine the value of x?
lesson 3. For 13.6 grams of Fe, FeO, Fe . mixture2O3 and Fe3O4 completely reacted with HNO . solution3 dilute (excess), get 1,344 liters of NO gas (the only reduction product, at dtc) and solution X. How many grams of anhydrous salt can be obtained from X?
Lesson 4. Mixture A consists of three iron oxides (FeO, Fe3O4Fe2O3) have the same number of moles. Dissolve all mg of this mixture A with HNO . solution3 then a mixture of K consisting of two NO . gases is obtained2 and NO has a volume of 1.12 liters (dktc) and the mass ratio of the mixture K to hydrogen is 19.8. What is the value of m ?
Lesson 5. For 2.16 grams of Mg react with HNO . solution3 residual. After the reaction occurs completely, 0.986 liters of NO gas (dktc) and solution X are obtained. Determine the mass of anhydrous salt obtained when the solution is depleted of X?
IV. Self-solution about Nitric Acid
Lesson 1. Completely dissolve 11.7 grams of Zn powder in HNO . solution3 Dilute solution A and a mixture of N . gas2female2O has a volume of 0.672 liters (dkc). Add excess NaOH to solution A and heat it to release gas, which reacts with 100 ml of 0.1 M HCl solution.
a. Write molecular and ionic equations for the reactions.
b. Calculate % by volume of gas mixture N2female2O.
Post 2. Completely dissolve 12 grams of mixture X including Al, Fe, Cu with HNO . solution3 The surplus is 6.72 liters (units) of a mixture of NO, NO . gases2 has a mass of 12.2 grams. Determine the mass of nitrate salt produced?
Lesson 3. Add 220 ml of HNO . solution3 react with 5 grams of Zn and Al mixture. The reaction releases 0.896 liters (units) of gases including NO and N .2O. The gas mixture has a vapor density relative to H2 is 16.75. After finishing the reaction, it was filtered to obtain 2.013 grams of metal.
a. How many grams of anhydrous salt can she get from solution A?
b. Calculate the concentration of HNO3 in the original solution?
Lesson 4. Dissolve completely mixture A consisting of x mol Fe and y mol Ag with mixed solution of HNO3 and THEY2SO4 there are 0.062 moles of NO gas and 0.047 moles of SO2 exit. Evaporate the solution after the reaction to obtain 22,164 grams of a mixture of anhydrous salts. What is the value of x and y?
Lesson 5. Let the mixture of Fe and Cu react with H . solution2SO4 excess dilution obtained 1.12 liters H2 (0 .)0C, 2 atm) to obtain solution A and insoluble solid B. To completely oxidize the insoluble solid B, 10.1 grams of KNO are required.3 produces a brown colorless gas in the presence of air and solution C. Calculate the mass % of each metal in the mixture.
Lesson 6. Add 1.92 grams of Cu powder to 100 ml of mixed solution X consisting of KNO3 0.16 M and H2SO4 0.5 M obtained solution A and only NO gas. To precipitate all Cu2+ in A a minimum of V liters of 0.5 M NaOH solution is required. What is the value of V?
V. Nitric Acid Multiple Choice Exercises
Question 1. HNO3 Can be used with any of the following substances:
A. NaHCO3CO2FeS, Fe2O3
B. KY2SO3KY2O, Cu, Fe(NO3)2
C. FeO, Fe2(SO)4)3FeCO3Na2O
D. CuSO4CuO, Mg3(PO .)4)2.
Verse 2. Cold concentrated nitric acid can react with which of the following substances?
A. Al, CuO, Na2CO3
B.CuO, Ag, Al(OH)3
C.P, Fe, FeO
D.C, Ag, BaCl2
Verse 3. Completely dissolve 0.9 g of metal X in the HNO . solution3 obtained 0.28 liters of N . gas2O (dktc). So X could be:
Verse 4. For FeO, Fe . substances2O3Fe(NO3)2, CuO, FeS. Number of substances that can react with HNO3 NO release is:
Question 5. Which of the following solutions cannot dissolve copper metal?
A. HNO solution3
B. Mixed solution of NaNO3+ HCl
C. FeCl . solution3
D. FeCl . solution2
Verse 6. To modulate HNO3 In the laboratory, which of the following chemicals is selected as the main raw material:
A. NaNO3H2SO4 special
B. WOMEN2 and THEY2
C. NaNO3female2H2 and HCl
D. AgNO3 and HCl
Verse 7. When Fe(III) oxide reacts with nitric acid, the products obtained are:
A. Fe(NO3)2NO, and THEY2O
B. Fe(NO3)2NO2and THEY2O
D. Fe(NO3)3 and THEY2O
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