Home
Class 10
CHEMISTRY
A 5.0 g sample of Cu (NO(3))(2).n(H(2)O)...

A 5.0 g sample of `Cu (NO_(3))_(2).n(H_(2)O)` is heated, and 3.9 g of the anhydrous salt remains. What is the value of 'n' ?

Text Solution

AI Generated Solution

To solve the problem, we need to find the value of 'n' in the hydrated copper nitrate formula \( Cu(NO_3)_2 \cdot nH_2O \). Here’s a step-by-step solution: ### Step 1: Write the reaction for dehydration When the hydrated copper nitrate is heated, it loses water to become anhydrous copper nitrate: \[ Cu(NO_3)_2 \cdot nH_2O \rightarrow Cu(NO_3)_2 + nH_2O \] ### Step 2: Identify given data - Mass of hydrated copper nitrate: \( 5.0 \, g \) ...
Promotional Banner

Topper's Solved these Questions

  • MOLE CONCEPT AND STOICHIOMETRY

    ICSE|Exercise WORKSHEET-1|10 Videos

  • MOLE CONCEPT AND STOICHIOMETRY

    ICSE|Exercise WORKSHEET-2|37 Videos

  • MOLE CONCEPT AND STOICHIOMETRY

    ICSE|Exercise ILLUSTRATIVE ASSIGNMENTS|28 Videos

  • ORGANIC CHEMISTRY

    ICSE|Exercise QUESTIONS FOR PRACTICE PAPER ON EXAMINATION PATTERN (ANSWER THE QUESTIONS)|40 Videos

Similar Questions

Explore conceptually related problems

A 5.0 g sample of Cu (NO_(3))_(2).n (H_(2)O) is heated, and 3.9 g of anhydrous salt remains. What is the value of 'n' ? Cu(NO_(3))_(2),n(H_(2)O)overset(Delta)toCu(NO_(3))_(2)+nH_(2)O

A 3.0 g sample of Na_(2)CO_(3).H_(2)O is heated to a constant mass. How much anhydrous salt remains ?

A 2.5 g sample of hydrate of Ca (NO_(3))_(2) was heated and only 1. 7 g of anhydrous salt remained. What percentage of water was in the hydrate ?

A 6.85g sample of the hydrated Sr(OH)_2.x H_2O is dried in an oven to given 3.13g of anhydrous sr(OH)_2. What is the value of x? (Atomic masses : Sr=87.60.O=16.0,H=1.0)

A 6.85g sample of the hydrated Sr(OH)_2.x H_2O is dried in an oven to give 3.13g of anhydrous Sr(OH)_2. What is the value of x? (Atomic masses : Sr=87.60.O=16.0,H=1.0)

A mixture of CuSO_(4).5H_(2)O and MgSO_(4).7H_(2)O was heated until all the water was driven off If 5.0g of mixture gave 3g of anhydrous salts, what was the percentage by mass of CuSO_(4).5H_(2)O in the original mixture :

From the equation : 3Cu + 8HNO_(3) to 3Cu (NO_(3))_(2) + 4H_(2)O + 2NO Calculate : mass of copper needed to react with 63 g of HNO_(3)

A sample of Na_(2)CO_(3).H_(2)O weighing 0.62 g is added to 10 ml of 0.1 N H_(2)SO_(4) solution . The resulting solution will be

A mixture of NH_(3(g)) and N_(2)H_(4_((g))) is placed in a sealed container at 300 K . The total pressure is 0.5 atm . The container is heated to 1200 K , at which time both substances decompose completely according to the equations: 2NH_(3(g))rarrN_(2(g))+3H_(2(g)) N_(2)H_(4_((g)))rarrN_(2(g))+2H_(2(g)) After decomposition is complete, the total pressure at 1200 K is found to be 4.5 atm . Find the amount (mole) per cent of N_(2)H_(4(g)) in the original mixture.

A 5-0cm^(3) solutions of H_(2)O_(2) liberates of 0.508g of iodine from acidified KI solution. Calculate the volume strength of H_(2)O_(2) at N.T.P.