Problem page suppose 25.1g of barium nitrate is dissolved in 200.ml of a 0.50 m aqueous solution of ammonium sulfate. calculate the final molarity of nitrate anion in the solution. you can assume the volume of the solution doesn't change when the barium nitrate is dissolved in it. round your answer to 3 significant digits.

1.26 M

Explanation:

The ion nitrate is NO₃⁻ and the Barium is from group 2 so it forms the ion Ba²⁺, so the barium nitrate has the formula: Ba(NO₃)₂. The molar masses are: Ba: 137 g/mol, N = 14 g/mol, O = 16 g/mol, so the molar mass of barium nitrate is:

137 + 2x(14 + 3x16) = 199 g/mol

The number of moles is the mass divided by the molar mass, so:

n = 25.1/199 = 0.126 mol of Ba(NO₃)₂

In 1 mol of the salt, there are 2 moles of NO₃⁻, so the number of moles of nitrate is 0.252 mol. Nitrates formed with ammonium (that can react when the solid dissolves) and with elements from group 1 and 2 are completely soluble in water. So, the moles of nitrate will remain 0.252 mol.

The molarity is the number of moles divided by the volume (0.2 L):

[NO₃⁻]= 0.252/0.2 = 1.26 M

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

the mantle

explanation:

earth is divided into three layers: the crust or the outermost layer on which we live; the underlying, middle layer - the mantle - and the core (the innermost layer of earth).