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10 Nov 2019

NiCl2(aq)+2NaOH(aq)?Ni(OH)2(s)+2NaCl(aq)

1) How many milliliters of 0.165M NaOH are needed to react with34.5mL of 0.415M NiCl2?

2) How many grams of Ni(OH)2 are produced from the reaction of38.5mL of 1.78M NaOH?

Mg(s)+2HCl(aq)?MgCl2(aq)+H2(g)

3)How many milliliters of a 6.500M HCl solution are required toreact with 42.20g magnesium?

4) What volume of hydrogen gas, at 25.0 ?C and 689.3 torr, willform when 662mL of 4.76M HCl reacts with excess Mg?

5) How many g NO of gas can be produced from the reaction of129.0mL of 3.40M HNO3 and excess Cu?

3Cu (s) + 8HNO3 (aq) ? 3Cu(NO3)2 (aq) + 4H2O (l) + 2NO (g)

6) Calculate the final concentration of each of the followingdiluted solutions:

A) A 50.0mL sample of 8.00% (m/v) NaOH is diluted with water sothat the final volume is 200.0mL

B) A 8.00mL sample of 50.0% (m/v) acetic acid (HC2H3O2) solutionis added to water to give a final volume of 25.0mL .

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Related questions

Balance the following Chemical Equations:

____Fe(s) + ____H₂O(g) Â® ____Fe₃O₄(s) + ____H₂(g)

____C₂H₆(g) + ____O₂(g) Â® ____CO₂(g) + ____H₂O(g)

___ C₆H₁₄ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (g)

___ C₃H₈O₃ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (l)

___ NaN₃ (s) Â® ___ Na (s) + ___ N₂ (g)

__ C₃H₅N₃O₉ Â® __ CO₂ + ___ N₂ + ___ H₂O + ___ O₂

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H₂O(g) + C(s) â¶ CO(g) +H₂(g)

(B) 2KClO₃(s) â¶ 2KCl(s) +3O₂(g)

(D) Pb(NO₃)₂(aq) + H₂SO₄(aq) â¶ PbSO₄(s) + 2HNO₃(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H₃PO₄

(B) Al(OH)₃

6. Complete and balance the following acid-base equations:

(A) A solution of HClO₄ is added to a solution of LiOH.

(B) Aqueous H₂SO₄ reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)₂(aq) + HC₂H₃O₂(aq) â¶

(B) H₃PO₄(aq) + CaCl₂(aq) â¶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl₂ and H₂. Ans: 1.67 g Mg

9. H₂ is produced by the reaction of 118.5 mL of a 0.8775-M solution of H₃PO₄ according to the following equation: 2Cr + 2H₃PO₄ â¶ 3H₂ + 2CrPO₄. How many grams of H₂ are produced? Ans: .315 g H₂

10. Automotive air bags inflate when a sample of sodium azide, NaN₃, is very rapidly decomposed.

2NaN₃(s) â¶ 2Na(s) + 3N₂(g)

What mass of sodium azide is required to produce 2.6 ft³ (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN₃

11. Urea, CO(NH₂)₂, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO₂ produced by combustion of 1.00 x 10⁴ grams of CO₂?

CO₂(g) + 2NH₃(g) â¶ CO(NH₂)₂(s) + H₂O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H₂SO₄(l) â¶ HCl(g) + NaHSO₄(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO₃(s)â¶CaO(s) + CO₂(s)

Ans: 92.0 %

14. Citric acid, C₆H₈O₇, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C₁₂H₂₂O₁₁ + H₂O +3O₂ â¶2C₆H₈O ₇+ 4H₂O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O₂ react according to P₄+5O₂ â¶ P₄O₁₀?

(B) Calculate the percent yield if 10.0 g of P₄O₁₀ is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N₂ â¶ Li₃N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO₃ requires 20.22 mL of the AgNO₃ solution to reach the end point?

AgNO₃(aq) + NaCl(aq) â¶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO₃)₂ solution.

2Cl^â(aq) + Hg(NO₃)₂(aq) â¶ 2NO₃^â(aq) + HgCl₂(s)

What is the Cl^â concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO₃)₂(aq) to reach the end point?

Ans: 0.009636 M