If 45.0 mL of 0.250 M CaCl2 is added to 17.5 mL of 1.00 M AgNO3, what is the mass of the AgCl precipitate?
If 30.0 mL of 0.150 M CaCl2 is added to 31.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? ?g
show your calculation When 100 mL of 0.250 M AgNO3 is added to 150. mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) o 3.58 g O 8.96 g o 13.3 g 02.11g
If 30.0 mL of 0.150 M CaCl2is added to 29.5 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? g
Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M NaCl solution. (a) What mass of AgCl will form? g AgCl the tolerance is +/-2% (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. [Ag+] = × 10 M [NO3−] = × 10 M [Na+] = × 10 M [Cl−] = × 10 M (c) What percentage of the Ag+ ions have precipitated?...
50.0 mL of a 0.250 M AgNO3 solution and 50.0 mL of 0.400 M Na2CO3 solution are mixed. How much of the silver carbonate precipitate will be formed? 2 AgNO3 (aq) + Na2CO3 (aq) -> Ag2CO3 (s) + 2 NaNO3 (aq)
4) When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.500 M NH4CI, how many grams of AgCl are formed? (MM AgCI =143.32 g/mol) AgNO3(ag)+ NH4C| (aq) AgCl(s)+ NH4NO3(aq)
To a 250.0 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100 M AgNO3, 0.245 M NaBr, and 0.100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously What mass of AgBr would precipitate from this mixture? (Hint: The Ksp of AgBr is 5.4 x 10-13 and the Ky of Ag(CN)2-is 1.0 × 1021) Number g AgBr
Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an excess of AgNO3 solution is added resulting in the formation of 31.12g of the precipitate. Calculate the % by mass of NaCl and CaCl2 in the original mixture. Show all work.
How many grams of aspartame(C4H8N,Os), also known as Nutrasweet, are contained in 45.0 mL of a 0.250 M solution? Question 1 When aqueous solutions of CaCl2(aq) and Na, C02(aq) are mixed, the products are NaCl(aq) and CaCO3(s). What ar the spectator ions in this reaction?
A solution (75.0 mL) of 0.250 M NH3 is being titrated with 0.500 M HCl. Kb = 1.8x10–5 for NH3. What species are present, and what are their concentrations: (a) Before any HCl has been added? (b) When 17.5 mL HCl have been added? (c) After 37.5 mL HCl solution has been added? (d) After 45.0 mL HCl solution has been added? Can you please show all work?