What volume (ml) of 3.0 m naoh is required to react with 0.8024-g copper(ii) nitrate? what mass of copper(ii) hydroxide will form, assuming 100% yield?

The reaction between NaOH and Cu(NO₃)₂ is as follows

2NaOH + Cu(NO₃)₂ ---> 2NaNO₃ + Cu(OH)₂

Q1)

stoichiometry of NaOH to Cu(NO₃)₂ is 2:1

this means that 2 mol of NaOH reacts with 1 mol of Cu(NO₃)₂

the mass of Cu(NO₃)₂ reacted - 0.8024 g 

molar mass of Cu(NO₃)₂ is 187.56 g/mol

therefore the number of Cu(NO₃)₂ moles that have reacted

 - 0.8024 g/ 187.56 g/mol = 0.00427 mol

according to the stoichiometry , number of NaOH moles - 0.00427 mol x 2 

then number of NaOH moles that have reacted - 0.00855 mol

In a 3.0 M NaOH solution, 3 moles are in 1000 mL of solution

Then volume required for 0.00855 mol - 1000 x 0.00855 /3 = 2.85 mL

2.85 mL of 3.0 M NaOH is required for this reaction

Q2) 

Assuming that there's 100 % yield of Cu(OH)₂ , we can directly calculate the mass of Cu(OH)₂ formed from the number of moles of reactants that were used up. 

Stoichiometry of Cu(NO₃)₂ to Cu(OH)₂ is 1:1

this means that 1 mol of Cu(NO₃)₂ gives a yield of  1 mol of Cu(OH)₂

the number of Cu(NO₃)₂ moles that reacted - 0.00427 mol 

Therefore an equal amount of moles of Cu(OH)₂ were formed

Then amount of Cu(OH)₂ moles produced - 0.00427 mol

Mass of Cu(OH)₂ formed - 0.00427 mol x 97.56 g/mol = 0.42 g 

A mass of 0.42 g of Cu(OH)₂ was formed in this reaction.

2b2t

explanation:

2b2t

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.