Show and prove that, by adding more cl will make ka even smaller, further [H+] decreases as equilibrium shifts to the left, as H+ ions are being used up, pH expected increases, is incorrect using the common ion effect
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![Show and prove that, by adding
more cl will make ka even
smaller, further [H+] decreases as
equilibrium shifts to the left, as
H+ ions are being used up, pH
expected increases, is incorrect
using the common ion effect](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3af3d195-4e67-4428-8e4f-5d80aaa997cb%2Fb002a996-ddd7-4088-a26e-551982d39ae4%2Fxb8g6ej_processed.jpeg&w=3840&q=75)
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- Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995A 0.150 mol quantity of CoCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Co²+ ions at equilibrium? Assume the formation constant* of Co(NH,+ is 5.0 × 1031M-6. concentration:Calculate the mas of AgCl need to contain 7.5g Ag
- In the solution AgSCN, what ion has a conflicting equilibrium due to pH considerations and what ion has a conflicting equilibrium due to the presence of a complexing agent?- adding the Fe(NO3)3 to the solution of iron (III) with the thiocyanate ion (SCN-): turns to darker red - adding the NaOH to the on of iron (III) with the thiocyanate ion (SCN-): faded to lighter red -adding KSCN to the solution of iron (III) with the thiocyanate ion (SCN-): turns to darker red Question: 1) Explain the result and how it happened. 2) State also the relationship and mechanism of equilibrium shift and complex ion reaction.9 What would happen to the solubility of CSSO, in water if the pH were decreased? Explain. 10 BIUA Y IEEE X² Paragraph What is the pH of a solution made by mixing 250 mL of 0.025 M HNO, and 100 mL of 0.05 M NaOH? Type your answer...
- For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K,, data in the ALEKS Data tab. compound CaCO, Cal, AgCN Does solubility change with PHY Oves Ⓒyes O no Ⓒyes One pH=9 O highest solubility pH = 8 X O O pH = 6 O ?Consider a beaker containing a saturated solution of PbI2in equilibrium with undissolved PbI2(s). Now solid KI isadded to this solution. (a) Will the amount of solid PbI2 atthe bottom of the beaker increase, decrease, or remain thesame? (b) Will the concentration of Pb2 + ions in solutionincrease or decrease? (c) Will the concentration of I- ionsin solution increase or decrease?A buffer solution contains 0.487 M CH,NH,Cl and 0.252 M CH,NH, (methylamine). D the pH change when 0.058 mol KOH is udded to 1.00 Lof the buffer. etemine pH ater addition - pli before addition- pH change-( Submit Answer Retry Entire Group more group attempts remaining Determine the pHi change when 0.080 mol HCIO, is added to 1.00 Lof a buffer solution that is 0.340 M in CH,COOH and 0.283 M in CH,COO". pH after addition - pH before addition pl change -[ Submit Answer Retry Entire Group 9 more group attempts remaining
- Explain the role of buffers in thecontrol of blood pH under variousconditions.When 38.0 mL of 0.1250 M H,SO̟ is added to 100. mL of a solution of PbI,, a precipitate of PbSO, forms. The PbSo, is then filtered from the solution, dried, and weighed. If the recovered PbSo, is found to have a mass of 0.0471 g, what was the concentration of iodide ions in the original solution Select one: а. 1.55 х 10 M -3 b. 1.55 x 10 M -3 с. 6.20 х 10 -3 d. 3.11 x 10 M -4 e. 3.10 x 10 M ΣΣAt what pH will FelO0, precipitate from a 0.06000 M Fe" solution? K 2800x10 At what pH will HgIOH); precipitate from a 0.06000 M Hg" solution? K 3.100x1o Which hydroxide precipitates at a lower OH concentration? Choose one O HelOH) 2 O Cannot be determined U Cannot be determinea In a solution buffered to a pH of 3.00, what is (Fe"VIHg" Is the separation of Hg" from Fe" "complete" in a solution buffered to a pH of 3.00? Choose one: O Yes O No O Cannot be determined