Question

1. What volume of 2.25 M nitric acid is needed to convert 9.0 g of m-chlorophenol...

1. What volume of 2.25 M nitric acid is needed to convert 9.0 g of m-chlorophenol to
3-chloro-4,6-dinitrophenol? (No excess of nitric acid is used.)

Homework Answers

Answer #1

3-chloro-4,6-dinitrophenol is C6H3ClN2O5

Molar mass of C6H3ClN2O5,

MM = 6*MM(C) + 3*MM(H) + 1*MM(Cl) + 2*MM(N) + 5*MM(O)

= 6*12.01 + 3*1.008 + 1*35.45 + 2*14.01 + 5*16.0

= 218.554 g/mol

mass(C6H3ClN2O5)= 9.0 g

number of mol of C6H3ClN2O5,

n = mass of C6H3ClN2O5/molar mass of C6H3ClN2O5

=(9.0 g)/(218.554 g/mol)

= 4.118*10^-2 mol

for 1 mol of C6H3ClN2O5, 2 mol of HNO3 is required

So,

mol of HNO3 required = 2*4.118*10^-2 mol

= 8.236*10^-2 mol

Now use:

mol of HNO3 = M(HNO3)*V(HNO3)

8.236*10^-2 mol = 2.25 M * V

V = 0.0366 L

V = 36.6 mL

Answer: 36.6 mL

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Nitric acid (HNO3), a strong acid, is formed in the following reaction. 2 NO(g) + 3/2...
Nitric acid (HNO3), a strong acid, is formed in the following reaction. 2 NO(g) + 3/2 O2(g) + H2O(g) → 2 HNO3(g). Assume a volume of 22.4 mL of NO gas (at STP = 1 atm, 273 K) completely reacts with excess of oxygen and water. If all of the acid that is formed is dissolved into 50. mL of water, what should be the pH of the solution? (pH = - log[H+])? A) 1.0 B) 1.7 C) 2.0 D)...
What volume of 12.0 M nitric acid is required to prepare 4.63 L of 0.200 M...
What volume of 12.0 M nitric acid is required to prepare 4.63 L of 0.200 M nitric acid ? Determine the concentration (molarity) of a solution made by dissolving 35.5 g of sodium sulfide in 550.0 mL of solution Consider the following reaction : 25.0mL of a 0.130 M sodium sulfate solution is reacted with 35.0 mL of a 0.124 M lead (ll) nitrate solution. The solvent for both solutions is water. If the reaction is carried out, what mass...
Determine the volume of 15.0 M sulfuric acid needed to react with 45.0 g of aluminum...
Determine the volume of 15.0 M sulfuric acid needed to react with 45.0 g of aluminum sulfate. Determine the % yield if 112 g of aluminum sulfate is produced under the above conditions.
What volume (in mL!!!) of 2.25 M HCl is required to react with 2.03 g of...
What volume (in mL!!!) of 2.25 M HCl is required to react with 2.03 g of zinc (65.41 g/mol) according to the following reaction? Zn(s) + 2 HCl (aq) → ZnCl2(aq) + H2(g)
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in...
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) What is the maximum mass of H2O that can be produced by combining 21.6 g of each reactant? STRATEGY: Convert 21.6 g NH3 to moles, then find the corresponding amount of H2O. Convert 21.6 g O2 to moles, then...
What volume of 12.0 moles nitric acid is required to prepare 6.11 L of 0.100 moles...
What volume of 12.0 moles nitric acid is required to prepare 6.11 L of 0.100 moles nitric acid ? A)0.196 B)19.6 c)0.611 d)0.0509 e) 1.96 What volume of 18.0 mole so forecast said is required to prepare 28.2 L of 0.126 mole. H2So4 A)5.07 B)0.197 C)508 D)3.55 E) 224 103.8 g sample nitric acid solution that is 70% HNO3 (by mass) contains A 72.7 B 1.15 C 1.65 D 5.27 E none of these
A 9.89 g sample of an aqueous solution of nitric acid contains an unknown amount of...
A 9.89 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 17.8 mL of 0.906 M barium hydroxide are required to neutralize the nitric acid, what is the percent by mass of nitric acid in the mixture? % by mass
A 11.7 g sample of an aqueous solution of nitric acid contains an unknown amount of...
A 11.7 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 28.6 mL of 6.48×10-2 M sodium hydroxide are required to neutralize the nitric acid, what is the percent by mass of nitric acid in the mixture?
QUESTION 1 What volume of 0.10 mol/L sulfuric acid is needed to create 50 mL of...
QUESTION 1 What volume of 0.10 mol/L sulfuric acid is needed to create 50 mL of a 0.080 mol/L solution? 50 mL 40 mL 1 L 10 mL 20 points    QUESTION 2 Solution 1 contains Malonic acid and 0.020 mol/L Manganese (II) sulfate monohydrate. What mass of Manganese (II) sulfate monohydrate (MW = 169 g/mol) should you weigh to prepare a final volume of 25.0 mL of solution 1? 0.084 g of MnSO4. H2O 140 g of MnSO4. H2O...
A 12.72 g sample of silver ore was treated with nitric acid to dissolve the silver....
A 12.72 g sample of silver ore was treated with nitric acid to dissolve the silver. After filtering, it was made to a volume of 250mL. 25mL of this sample was treated with 50mL of 0.1011M potassium chloride, which precipitated all the silver and left chloride in excess. The excess chloride was titrated with 0.0871M silver nitrate solution, and required 15.69mL. Calculate the percent of silver in the ore