World News Headlines

Coverage of breaking stories

For which of the following mixtures will Ag2SO4(s) precipitate?

source : yahoo.com

For which of the following mixtures will Ag2SO4(s) precipitate?

The solubility product for Ag2SO4 is Ksp = 1.4*10^-5

The definition of Ksp is Ksp = [Ag+]²*[SO4^2-]

For each solution, compute [Ag+] and [SO4^2-]

if the product formed is < Ksp. there will be no precipitate

Na2SO4(aq) + 2AgNO3(aq) ———> Ag2SO4(s?) + 2NaNO3(aq)

one mole of Na2SO4 reacts with 2 moles of AgNO3 to produce one mole of Ag2SO4

mole ratio Ag2SO4/AgNO3 = 1/2

150 mL 0.10 M Na2SO4 = 0.0150 mol Na2SO4

5.0 mL of 0.20 M AgNO3 = 0.001 mol AgNO3

AgNO3 is the limiting reactant, so 0.001 mol of it reacts, forming 0.0005 mole Ag2SO4

in 155 mL of solution, so

[Ag2SO4] = 0.003226 M

then

[Ag+] = 0.006452 M

[SO4^2-] = 0.003226 M

0.006452²*0.003226 = 1.34*10^-7

This is < Ksp, so no precipitate is formed.

150 mL 0.10 M Na2SO4 = 0.0150 mol Na2SO4

5.0 mL of 0.30 M AgNO3 = 0.0015 mol AgNO3

AgNO3 is the limiting reactant, so 0.0015 mol of it reacts, forming 0.00075 mole Ag2SO4

in 155 mL of solution, so

[Ag2SO4] = 0.004839 M

then

[Ag+] = 0.009677 M

[SO4^2-] = 0.004839 M

0.009677²*0.004839 = 4.53*10^-7

This is < Ksp, so no precipitate is formed.

150 mL 0.10 M Na2SO4 = 0.0150 mol Na2SO4

5.0 mL of 0.40 M AgNO3 = 0.002 mol AgNO3

AgNO3 is the limiting reactant, so 0.002 mol of it reacts, forming 0.001 mole Ag2SO4

in 155 mL of solution, so

[Ag2SO4] = 0.01290 M

then

[Ag+] = 0.02581M

[SO4^2-] = 0.01290 M

0.02581²*0.01290 = 8.59*10^-6

This is < Ksp, so no precipitate is formed.

150 mL 0.10 M Na2SO4 = 0.0150 mol Na2SO4

5.0 mL of 0.50 M AgNO3 = 0.0025 mol AgNO3

AgNO3 is the limiting reactant, so 0.0025 mol of it reacts, forming 0.00125 mole Ag2SO4

in 155 mL of solution, so

[Ag2SO4] = 0.008065 M

then

[Ag+] = 0.01613 M

[SO4^2-] = 0.008065 M

0.01613²*0.008065 = 2.1*10^-5

This is > Ksp, so a precipitate will be formed.

How to Write the Net Ionic Equation for... - YouTube

How to Write the Net Ionic Equation for… – YouTube – Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). Another option to determine if a precipitate forms is to have memorized the solubility rules. In this reaction, Ag2SO4 will be insoluble and will be a precipitate…Calculate (Ag^+) and (SO4^2-), substitute into Ksp expression. That is Qsp. If Qsp > Ksp a ppt will occur. Name the separation techniques which you will apply for the separation of the following mixtures : asked Nov 21, 2017 in Class IX Science by ashu Premium (930 points).Now #Q">>"K_"sp"=2.93xx10^-13#…and so precipitation will occur. And now you use the same procedure on all the other examples. You could post them here….

for which of the following mixtures will ag2so4(s) precipitate? – For which of the mixtures will Ag2SO4(s) precipitate? Find the Ksp values for Al(OH)3 and Pb(OH)2 in the chempendix. Answer: [Pb 2+] = = 0.00147 M Explanation: **Ksp of lead(II) sulfate (PbSO4) 2.53 x 10^-8 **Ksp of strontium sulfate (SrSO4) 3.44 x 10^-7 **the reactions to consider: (1)…Two portable PA-S potentiometric analyzers (Ural State University of Economics, Yekaterinburg, Russia) were used for potentiometric measurements. The standard two-electrode configuration of the potentiometric sensor system includes one indicator electrode and one reference electrode…Compounds are often found mixed with other compounds. Mixtures may be separated and analysed. Tests for anions. Testing for halide ions. The halogens are the elements in group 7 of the Periodic Table, and include chlorine, bromine and iodine.

for which of the following mixtures will ag2so4(s) precipitate?

Which of the following mixtures will result in the formation… | Socratic – SO. 4(s)⇌. 2Ag. + (aq)+. SO. Many of the pigments used by artists in oil-based paints (Figure 15.3) are sparingly soluble in water. For example, the solubility of the artist's pigment chrome yellow, PbCrO4, is 4.6.For which of the following mixtures will Ag2SO4(s) precipitate? a. 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) b. 150.0 A substance will only precipitate if it is not soluble in an aqueous solution. If you look at the solubility rules, it indicates that all sulfates are soluble except forPrecipitation titrations are based on reactions that yield ionic compounds of limited solubility. Only limited precipitating agents are used because of the slow rate of appearance of precipitate (Skoog, et al., 2014). In this reaction, the analayte and titrant form an insoluble precipitate that can serve as a…

PDF) Moderate-temperature Operable SO2 Gas Sensor Based On Zr4+ Ion  Conducting Solid Electrolyte
MARC Á. BONCZ
Solved: E CHEM 1A15 ISOn 19 11:59 PM A 19.7/100 Ren Print | Chegg.com
This Is A Special Equilibrium Constant Known As The “Solubility Product  Constant”.
PDF) NOHSO4/HF - A Novel Etching System For Crystalline Silicon
Water | Free Full-Text | Eggshell-supported Catalysts For The Advanced  Oxidation Treatment Of Humic Acid Polluted Wastewaters | HTML
PCCP PAPER
Method Development For Detecting And Characterizing Manufactured Silver  Nanoparticles In Soil Pore Water Using Asymmetrical Flow
Screen Shot 2019-11-15 At 9.12.13 PM.png - For Which Of The Mixtures Will  Ag2SO4(s Precipitate 150.0 ML Of 0.10 M NazSO4(aq And 5.0 ML Of 0.20 M |  Course Hero
Trace Metals Pollution Of Waters And Soils In Kardjali Region, Bulgaria |  SpringerLink
Highly Efficient Luminescent Solar Concentrators Based On  Benzoheterodiazole Dyes With Large Stokes Shifts - Gao - 2020 - Chemistry –  A European Journal - Wiley Online Library