Question

A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.10M NaI solution...

A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.10M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 25.5 g. Find the mass of AgI in the precipitate.

Homework Answers

Answer #1

mass balance:

Mass of AgI + mass of HGI2 = 25.5

mol balance:

mol of NaOH = MV = 1.1*0.1 = 0.11

mol of I- from AgI + mol of I- from HgI2 = 0.11

mol of AgI + 2*mol of HgI2 = 0.11

then, assume

"x" = mass of AgI

then, mass of HgI2 = (25.5-x)

MW of HgI2 = 454.4

MW of AgI = 234.77

apply mol balance:

mol of AgI + 2*mol of HgI2 = 0.11

mass of AgI/ MW of AgI = mol of AgI

mass of HgI2 / MW of HgI2 = mol of HgI2

mol of AgI + 2*mol of HgI2 = 0.11

mass of AgI/ MW of AgI + 2 * mass of HgI2 / MW of HgI2 = 0.11

substitute

x/ 234.77 + 2 * (25.5-x) / 454.4 = 0.11

solve for x

454.4 x + 2 * (25.5-x) *234.77 = 0.11*234.77 *454.4

454.4 x + 2 * (25.5-x) *234.77  = 11734.74

454.4x - 2*234.77 x + 2*25.5*234.77= 11734.74

x(454.4 + -2*234.77 ) = 11734.74-2*25.5*234.77

x = ( 11734.74-2*25.5*234.77)/(454.4 + -2*234.77 )

x = 15.754 g of AgI

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.24 M NaI...
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.24 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 28.7 g Find the mass of AgI in the precipitate.
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.49 M NaI...
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.49 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 34.4 g. Find the mass of AgI in the precipitate. Express your answer to two significant figures
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.44 M NaI...
A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.44 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 33.3 g. Find the mass of AgI in the precipitate. (I already tried 11.3g and it didn't work)
*A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.06 M NaI...
*A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.06 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 24.6 g . *Find the mass of AgI in the precipitate. Express your answer to two significant figures and include the appropriate units
A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.55 M...
A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.55 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 49.8 g . Find the mass of Cr3+ in the original solution.
A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.54 M...
A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.54 M NaF solution is required to cause the complete precipitation of these ions as CrF3 (s) and MgF2 (s). The total mass of the precipitate is 49.6 g. Find the mass in grams of Cr3+ in the original solution.
an aqueous solution contains 0.010M br and 0.010 M I. If AG+ is added until agbr(s)...
an aqueous solution contains 0.010M br and 0.010 M I. If AG+ is added until agbr(s) just begins to precipitate. what are the concentrations of ag and I? ksp of agbr = 5.4E-13, ksp of agi = 8.5E-17?
A basic solution contains the iodide and phosphate ions that are to be separated via selective...
A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.960 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. (Answer in mol/L) Calculate the minimum Ag+ concentration required...
A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2...
A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. You may want to reference (Pages 648 - 658) Section 16.2 while completing this problem. Part A Calculate the pH of the solution upon addition of 48.1 mL of 1.00 MHCl to the original buffer.
20.0 L of an aqueous solution of silver nitrate (AgNO3). 10.0 L of a 0.0500 mol...
20.0 L of an aqueous solution of silver nitrate (AgNO3). 10.0 L of a 0.0500 mol / L solution of calcium iodide (CaI2) is added thereto. At the end, all the Ag + ions precipitated and the molar concentration of the I ions is 0.0100 mol / L. a) What was the initial molar concentration of AgNO3? b) What mass of silver iodide has precipitated? c) What is the melting point of the final water (suppose 1 liter of solution...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT