# At T1 ℃, 5.6g iron powder was put into 100g copper sulfate solution to completely react   At T1 ℃, put 5.6g iron powder into 100g copper sulfate solution and filter after just complete reaction, so as to obtain: Mass of FeSO4 in filtrate The obtained filtrate was evaporated at a constant temperature to remove 66g of water and just turned into   Saturated solution at T1 ℃, find   Solubility of the solute at T1 ℃?

## At T1 ℃, 5.6g iron powder was put into 100g copper sulfate solution to completely react   At T1 ℃, put 5.6g iron powder into 100g copper sulfate solution and filter after just complete reaction, so as to obtain: Mass of FeSO4 in filtrate The obtained filtrate was evaporated at a constant temperature to remove 66g of water and just turned into   Saturated solution at T1 ℃, find   Solubility of the solute at T1 ℃?

Generated in filtrate   Feso4x g, y g CuSO4 participated in the reaction+       Fe=     FeSO4+       Cu   one hundred and sixty             fifty-six       152 &n...

### Put 100g iron bar into 200g copper sulfate solution with mass fraction of for a period of time, and the iron bar is 101.6g. Calculate the mass fraction of solute in the solution at this time

8g, the hexahydrate of the two chlorides can be obtained by combining with water, with a total of 88.8g. The mixture of the two hydrates is strongly burned into the mixture of oxides (gold C. 8W / 88g anhydrous copper sulfate is added D. 8W / 88g copper sulfate crystal is added for analysis: (8) set the evaporation solvent XG, and the concentration of the solvent is 1

### If sufficient iron powder reacts with 50g dilute sulfuric acid to generate 0.2g hydrogen, what is the solute mass fraction of dilute sulfuric acid used?

Fe + H2SO4 === FeSO4 + H2↑
98 2
x 0.2g
98/x=2/0.2g
x=9.8g
9.8g/50g*100%=19.6%

### The mixture of magnesium powder, zinc powder, aluminum powder and iron powder is 40g, which just completely reacts with a certain amount of dilute sulfuric acid with a mass fraction of 30%, and is obtained after steaming and drying

After the mixture is completely reacted with sulfuric acid, sulfate (including MgSO4, ZnSO4, Al2 (SO4) 3 and FeSO4) is obtained by evaporation. The mass of solid increase is the mass of sulfate. If the mass of dilute sulfuric acid solution is set as Mg, the mass of sulfate is 0.3m * 96 / 98 G, and the mass of solid after evaporation is (40 + 0.3m * 96 / 98) g

### The mixture AG of zinc powder, aluminum powder, iron powder and magnesium powder reacts exactly with a certain mass of dilute sulfuric acid with a solute mass fraction of 25%, and evaporates water to obtain solid C (excluding crystal water) BG. How many grams of H2 are generated in the reaction process?

The mass ratio of H2 and SO4 in H2SO4 is: 2:96 = 1:48;
The mass of sulfate = BG AG,
Let the mass of H2 generated in the reaction process be XG,
∴x
bg−ag＝1
48，
Solution: x = B − a
48g．
Answer: the mass of H2 generated during the reaction is B − a
48g．

### 3.8g of the mixture of zinc powder, aluminum powder, iron powder and magnesium powder reacts exactly with dilute sulfuric acid with a mass fraction of 25% solute. Evaporate the water of the reaction mixture to 11g of solid (excluding crystal water), and the mass of hydrogen generated in the reaction is () A. 0.15g B. 0.20g C. 0.30g D. 0.45g

According to the subject information, the mixture and sulfuric acid react exactly, so the sum of the mass of the mixture and pure sulfuric acid (H2SO4) is equal to the sum of the mass of the remaining solid and hydrogen. The mass of sulfate before and after the reaction = (11g - 3.8g) = 7.2g, then the mass of pure sulfuric acid = 7.2g ÷ 96
98 = 7.35g. Therefore, the mass of hydrogen = the mass of hydrogen element in sulfuric acid = 7.35g - 7.2g = 0.15g, so a