What mass of precipitate should be obtained by the reaction between masses of #115g# #AgNO_3(aq)# and #85g# of #BaCl_2# where each of the components are dissolved in water?

Answer 1

Approx. #100*g# #AgCl# precipitate should deposit........

A stoichiometric equation is first required.

#2AgNO_3(aq) + BaCl_2(aq) rarr 2AgCl(s)darr +Ba(NO_3)_2#

Silver chloride is as soluble as a brick and separates from aqueous solution as a curdy white precipitate, in contrast to nitrates and most halides, which are soluble.

Thus, we calculate equivalent amounts of barium chloride and silver nitrate.

"Moles of silver nitrate" are equal to (115g)/(169.87gmol^-1) = 0.677mol.

#"Moles of barium chloride"=(85*g)/(208.23*g*mol^-1)=0.408*mol# with respect to barium chloride; but #0.816*mol# with respect to chloride ion. Are you with me?

And thus, because chloride is in excess, we should achieve stoichiometric precipitation of silver chloride, i.e. #0.677*mol# #AgCl#.

And tis represents a mass of #0.677*molxx143.32*g*mol^-1#

#=??*g#

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Answer 2

Wyatt Adkins

The mass of precipitate obtained by the reaction between 115 g of AgNO3 and 85 g of BaCl2, where each component is dissolved in water, can be calculated using stoichiometry. The balanced chemical equation for the reaction is:

2AgNO3(aq) + BaCl2(aq) -> 2AgCl(s) + Ba(NO3)2(aq)

Using the molar masses: AgNO3 = 169.87 g/mol BaCl2 = 208.23 g/mol AgCl = 143.32 g/mol

First, calculate the number of moles of each reactant: moles of AgNO3 = mass / molar mass = 115 g / 169.87 g/mol moles of BaCl2 = mass / molar mass = 85 g / 208.23 g/mol

Next, determine the limiting reactant by comparing the moles of each reactant and their stoichiometric coefficients in the balanced equation.

Then, use the stoichiometry of the reaction to find the mass of AgCl precipitate formed from the limiting reactant.

Finally, calculate the mass of AgCl precipitate using the molar mass of AgCl.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

What mass of precipitate should be obtained by the reaction between masses of #115*g# #AgNO_3(aq)# and #85*g# of #BaCl_2# where each of the components are dissolved in water?

What mass of precipitate should be obtained by the reaction between masses of #115g# #AgNO_3(aq)# and #85g# of #BaCl_2# where each of the components are dissolved in water?