A.How many moles of silver carbonate can be made from 50.0 ml of 0.100 M AgNO3...

A.How many moles of silver carbonate can be made from 50.0 ml of 0.100 M AgNO3 and 50.0 ml of 0.100 M Na2CO3 ? B. What is the molarity of the carbonate ions left over? (First find how many moles of carbonate are left over.) C. What is the molarity of the sodium ions in the final solution?.

Expert Solution

2 AgNO3 (aq) + Na2CO3 (aq) --------> 2 NaNO3 (aq) + Ag2CO3 (s)

number of moles of AgNO3 = 50 * 0.1 /1000 = 5 *10^-3 moles

number of moles of Na2CO3 = 50 * 0.1 /1000 = 5 * 10^-3 moles

2 moles of AgNO3 requires 1 mole of Na2CO3

5 * 10^-3 moles of AgNO3 requires (1/2) * 5 *10^-3 moles of Na2CO3

= 2.5 * 10^-3 moles of Na2CO3

remaining moles of Na2CO3 = 5 *10^-3 - 2.5 *10^-3

= 2.5 * 10^-3

concentration of Na2CO3 = 2.5 *10^-3 * 1000/ (50 +50) = 0.025 mol /L

molarity of CO3 2- ions = 0.025 mol /L

molarity of Na+ ions = 0.025* 2 = 0.05 mol /L

queen_honey_blossom answered 2 years ago

A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of 0.100 M...

A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the resulting solution. The Ksp value for AgIO3(s) is 3.17 × 10-8. [Ag+] =____ mol/L

Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of 0.100 M...

Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of 0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5. a. Calculate the pH of both solutions before mixing. b. Construct an ICE table representative of this mixture. c. Determine the approximate pH of the solution. d. Determine the percent ionization of the acetic acid in this mixture

50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate...

50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate the concentration of Ag + and Cl- in the resulting solution, assuming the volumes are additive. Ksp(AgCl) = 1.82*10-10

50.0 mL of a 0.100 -M HoAc solution is titrated with a 0.100 -M NaOH solution....

50.0 mL of a 0.100 -M HoAc solution is titrated with a 0.100 -M NaOH solution. Calculate the pH at each of the following points. Volume of NaOH added: 0, 5, 10, 25, 40 ,45 , 50 , 55 , 60 , 70 , 80 , 90 , 100

If 30.0 mL of 0.150 M CaCl2 is added to 35.0 mL of 0.100 M AgNO3,...

If 30.0 mL of 0.150 M CaCl2 is added to 35.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate?

75.0 mL of 0.200 M AgNO3 is combined with 125.0 mL of 0.100 M Nacl. solid...

75.0 mL of 0.200 M AgNO3 is combined with 125.0 mL of 0.100 M Nacl. solid AgCl forms. a) what mass of AgCl forms ? b) what is the concentration of each of the 4 ions in the final solution ? assume that volumes are additive. note.... none of the concentration will be zero.' -Ag , Na , NO3 and Cl

A 50.0 ml sample of 0.100 M Ba (OH)2 is treated with 0.100 M HNO3. Calculate...

A 50.0 ml sample of 0.100 M Ba (OH)2 is treated with 0.100 M HNO3. Calculate the ph after the addition of the following volumes of acid. a). 25 ml of HNO3 b). 50 ml of HNzo3 c). 75 ml of HNO3 d). 100 ml of HNO3 e). 125 ml of HNO3

if 22.8 ml of 0.100 m mgcl2 is needed to completely react 15.0 ml of agno3...

if 22.8 ml of 0.100 m mgcl2 is needed to completely react 15.0 ml of agno3 solution, what is the molarity of the agno3 solution? the reaction is: mgcl2(aq)+2 agno3(aq)->2 afcl(s)+mg(no3)2(aq) A. 0.0760 m B. 0.152 m C. 0.304 m

a) A beaker contains 200.0 mL of 0.250 M AgNO3. 200.0 mL of 0.100 M HCl(aq)...

a) A beaker contains 200.0 mL of 0.250 M AgNO3. 200.0 mL of 0.100 M HCl(aq) is added to it. What is the NO3− concentration in the final mixture?b) What is the Ag+(aq) concentration in the final mixture? (Hint: does anything happen when you mix these solutions?)

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide,...

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide, determine the pH when: (a) 50.0 mL of base has been added. (b) 75.0 mL of base has been added. (c) 100.0 mL of base has been added.

Question