A metal M forms the sulphate `M_(2)(SO_(4))_(3)`. A 0.596 gram sample of the sulphate reacts with excess `BaCl_(2)` to give 1.220 g `BaSO_(4)`. What is the atomic mass of M ?

A metal M forms the sulphate M_2(SO_4)_3. A0.596 gram sample of the sulphate reacts with excess BaCI_2 to given 1.220g BaSO_4 . What is the atomic mass of M? (Atomic mass : S=32, Ba=137.3 )

A metal M forms the sulphate M_2(SO_4)_3. A0.596 gram sample of the sulphate reacts with excess BaCI_2 to given 1.220g BaSO_4 . What is the atomic mass of M? (Atomic mass : S=32, Ba=137.3 )

A metal M forms the sulphate M_2(SO_4)_3. A0.596 gram sample of the sulphate reacts with excess BaCI_2 to given 1.220g BaSO_4 . What is the atomic mass of M? (Atomic mass : S=32, Ba=137.3 )

A metal M forms the sulphate M_2(SO_4)_3 0.596 gm of the sample reacts with excess BaCl_2 to give, 1.22 gm BaSO_4 . What is the atomic weight of the M ? (S = 32, Ba + 137.3)

A sample is a mixture of Mohr's salts and (NH_(4))_(2)SO_(4). A 0.5 g sample on treatment with excess of BaCl_(2) solution gave 0.75 g BaSO_(4) . Determine percentage composition of the salt mixture. What weight of Fe_(2)O_(3) would be obtained if 0.2 g of the sample were ignited in air?

A sample is a mixture of Mohr's salts and (NH_(4))_(2)SO_(4). A 0.5 g sample on treatment with excess of BaCl_(2) solution gave 0.75 g BaSO_(4) . Determine percentage composition of the salt mixture. What weight of Fe_(2)O_(3) would be obtained if 0.2 g of the sample were ignited in air?

The sulphate of a metal has the formula M_(2)(SO_(4))_(3) . The formula for its phosphate will be

What is the normality of sulphate ions in 1M Al_(2)(SO_(4))_(3) solution?

What type of reaction is this : Na_(2)SO_(4)+BaCl_(2) to BaSO_(4)+2NaCl