A student produced a soluble salt by reacting copper(II) carbonate with dilute nitric acid.
This is the method used:
Complete the word equation for the reaction: copper(II) carbonate+nitric acid→_______________+_______________+carbon dioxide\text{copper(II) carbonate} + \text{nitric acid} \rightarrow \text{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_} + \text{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_} + \text{carbon dioxide}copper(II) carbonate+nitric acid→_______________+_______________+carbon dioxide
Give one observation the student could make during Step 4 which shows that the copper(II) carbonate is in excess.
Give one reason for filtering the mixture in Step 5.
Name the equipment that can be used to warm the filtrate gently in Step 6.
The maximum theoretical mass of the salt that could be produced using 40 cm340\text{ cm}^340 cm3 of the nitric acid is 6.8 g6.8\text{ g}6.8 g. The percentage yield of the copper(II) nitrate salt is 72.5%72.5\%72.5%. Calculate the mass of salt actually produced. Use the equation: percentage yield=mass of salt actually producedmaximum theoretical mass of salt that could be produced×100\text{percentage yield} = \frac{\text{mass of salt actually produced}}{\text{maximum theoretical mass of salt that could be produced}} \times 100percentage yield=maximum theoretical mass of salt that could be producedmass of salt actually produced×100
Some salts can be produced by reacting a metal with a dilute acid. Neither platinum nor sodium is used to produce a salt with dilute nitric acid. Give one reason why each metal is not used: