# Chemistry

Calculate the molar masses of copper (II) nitrate trihydrate and of the precipitate formed by this reaction.

Are these steps right?

Molar mass of Copper: (Cu 2+) 63.55
Molar mass of Nitrate: (NO3 -) 62.01
Copper(II) Nitrate Formula = Cu(No3)2
Molar Mass of Copper(II) Nitrate =(62.01 x 2 = 124.02) (124.02 + 63.55 = 187.57) 187.57

trihydrate: 3H2O - Molar Mass of H2O: 18.02 x 3 = 54.06

**Total Molar mass of Copper(II) Nitrate trihydrate = 241.63g

**Mass of precipitate (Cu(OH)2): 97.57g

1. 👍 0
2. 👎 0
3. 👁 132
1. All ok.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

1) Write a balanced chemical equation for the reaction between Cu(NO3)2 * 3 H2O and NaOH. Underline the formula for the precipitate produced by this reaction. (The water of hydration in Cu(NO3)2 * 3 H2O appears as liquid water on

asked by Sarah on May 17, 2010
2. ### Chemistry

Write a balanced formula equation with phase indicators: Strong heating of copper(II) nitrate trihydrate produces copper (II) oxide, nitrogen dioxide, oxygen gas, and water (The part I'm confused about is how to write the

asked by Kyla on November 16, 2014
3. ### chemistry

A 0.8552g sample of copper alloy is treated with 8 molar nitric acid and filtered and the precipitate is ignited giving a residue of 0.0632g of SnO2. The zinc is determined in one half of the filterate by precipitating it as

asked by william on September 15, 2017
4. ### Chemistry Lab

Are you titrating? Qualitative testing? Just what? If the copper is in solution you can filter the ppt (or let the ppt settle and decant some of the supernatant liquid) and to the filtrate or the decanted liquid add some more NaOH

asked by Joe on October 9, 2008
5. ### chemistry

If you had left your copper(II) nitrate/potassium hydroxide precipitate stand for a while, the precipitate would turn into a black powder. The copper doesn’t reduce in this reaction, but one mole of water is produced from the

asked by Cortney on April 23, 2015
6. ### Chemistry

4) Using your initial mass of copper (0.38), calculate the minimum volume of concentrated 12M nitric acid needed to completely react with your copper to form copper (II) nitrate 5) Using your answer from question 4 (2x10^-3 L),

asked by Anonymous on September 22, 2014
7. ### Chemistry

24.0 mL of 2.4 M silver nitrate is mixed with 32.0 mL of 2.0 M sodium chloride. ( I wrote the balanced equation as AgNo3+NaCl -> NaNo3 + AgCl ) A) Identify the precipitate formed by name and formula. - I wrote AgCl (silver

asked by Sara on March 2, 2016
8. ### Chemistry

Copper dissolves in nitric acid, producing copper (ll) nitrate. After reaction with sodium hydroxide and heating, copper nitrate changes to copper (ll) oxide. Calculate the percent yield of this process if 1.235 g of copper

asked by Raj on October 28, 2007
9. ### Chemistry

A student was given a solid containing a mixture of nitrate salts. The sample completely dissolved in water, and upon addition of dilute HCl, no precipitate formed. The pH was lowered to about 1 and H2S was bubbled through the

asked by Neeta on April 10, 2014
10. ### Chemistry

Assuming an efficiency of 38.60%, calculate the actual yield of magnesium nitrate formed from 145.9 g of magnesium and excess copper(II) nitrate. I got 230.5g but it isn't right.. I got 6 mols of Mg then calculated molar mass of

asked by Clare on April 22, 2014

More Similar Questions