General Chemistry Answers

How do you get 0.501 M with 41.0 mL and 3.41M and 279mL

2NaCl + MgO -> Na2O+ MgCl2

The mass of magnesium oxide resulting from the combustion of 8 g of the element magnesium

How many moles of oxygen (O₂) are needed to react with 56.8 grams of ammonia?

4 NH3 + 5 O2 → 4 NO + 6 H2O 

 How many grams of solute are present in each of these solutions?

a.    37.2 mL of O.471 M HBr

Argon has three naturally occurring isotopes, argon-36 (atomic mass=35.97 u), argon-38 (atomic mass=37.96 u), and argon-40 (atomic mass= 39.96 u).The natural abundance of argon-36 is 0.334%, and abundance of argon-38 is 0.063%.                                                                   Determine the average atomic mass of argon.  Show all work. 

Which of the following statements are correct for the following oxidation-reduction reaction: Fe²⁺ (aq) + Cu²⁺ (aq) → Fe³⁺ (aq)+ Cu (s)

• i. Fe²⁺ gains electrons, Fe²⁺ is reduced
• ii. Cu²⁺ gains electrons, Cu²⁺ is reduced
• iii. Cu gains electrons, Cu is reduced
• iv. Fe²⁺ loses electrons, Fe²⁺ is oxidized 
• v. Fe²⁺ is an oxidizing agent
• vi. Cu²⁺ is an oxidizing agent

20.0mL of HCl was just neutralized by 25.0mL of a solution of KOH with a concentration of 0.500mol/L. Write the balanced equation of the neutralization reaction and determine the molar concentration of hydrochloric acid.

A volume of 25.0 mL of 1.9752M strong monoprotic acid, HA, is to be titrated with 0.4115M strong base, B(OH)2. Answer the questions that follow and Write answer in THREE SIGNIFICANT FIGURES with complete solution.

A. Calculate the volume of the base titrant (in milliliters) required to reach the equivalence point.

B. Calculate the pH of the resulting solution when the original solution has been titrated with 50.0 mL of the base titrant

Calculate the pH of the resulting solution when the original solution has been titrated with 50.0 mL of the base titrant.

C. Calculate the pH of the resulting solution when the original solution has been titrated with 55.0 mL of the base titrant. 

D. Calculate the pH of the resulting solution when the original solution has been titrated with 60.0 mL of the base titrant.

E. Calculate the pH of the resulting solution when the original solution has been titrated with 65.0 mL of the base titrant.

2. Calculate the pressure (in mmHg, density of Hg =13.6g/ml)) for a column of water( density of H2O=1.0g/ml) that is 6.0 m high(1.0m=1000mm):