When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 x 10-4) and O.250 M (CH3)2NH2NO3 . What is the pH…

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Q: What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 6.2 x 10-2?…

A: Molar solubility is defined as the number of moles of solute dissolve into solution.

Q: During a titration, the pH of an analyte solution containing HA(aq) is 5.56 and the ratio of (A…

A: Given  pH of solution is 5.56 ratio of [A-]/[HA] is .842 we have to determine Ka

Q: The Kp value for Al(OH)3 is 3.0 x 10-34. Part 1 You answered correctly! Move on to the next part.…

A: Given : Al(OH)3 of the Ksp = 3.0 ×10-34 PH = 9.59   Finds : To calculate the Molar solubility of…

Q: Calculate the molar solubility (in mol/L) of Ag2S(s) at 25 °C in a solution of 0.30 M Na2S(aq).  Ksp…

A: The majority of ionic compounds are water-soluble. When a substance is soluble, it dissociates into…

Q: If the equilibrium constant for a reaction A + B 2C is measured as Keq = 1.318. What would the…

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Q: Calculate the Molar Solubility of aqueous Barium sulfate at 20 oC in a solution of 0.0100 M Na2SO4.…

A: Molarity of Na2SO4 = 0.0100 M Therefore, [SO4]2- in solution initially = 0.0100 M BaSO4 (s)…

Q: Sodium sulfate is slowly added to a solution containing 0.0500 M Ca²+ (aq) and 0.0210 M Ag+ (aq).…

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Q: Calculate the pH during the titration of 30 mL of 0.1000 M C2H4COOH(aq) with 0.1000 M NaOH(aq) after…

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Q: Write a balanced net ionic equation to show why the solubility of AgOH(s) increases in the presence…

A: The net ionic equation shows only the species that are involved in the reaction. Ksp for AgOH = 2.0…

Q: Calculate the molar solubility of iron(II) hydroxide in an aqueous solution buffered at pH = 6.07.

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Q: Given the equation Ag*(aq) + 2 NH3 (aq) → [Ag(NH3),]*(aq) K = 2.00 × 107 determine the concentration…

A: Ksp of AgCl = 1.77 × 10-10  Kf = 2.00 × 107 Mass of AgCl = 767 mg = 0.767 g Volume = 100.0 mL =…

Q: What is the pH of a buffer made of 1.4E-1 M CH3COOH(aq) and 4.6E-1 M NaCH3COO(aq)? Ka for CH3COOH =…

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Q: Consider the titration of 300.0 mL of 0.450 M NH3 (Kb = 1.8  10–5) with 0.450 M HNO3. At the…

A: pH of an aqueous solution of a salt of a weak base and strong acid = 7 - (pKb + logC)/2 Where, pKb =…

Q: Calculate the pH of (a) 0.10 M NH4CI(aq), (b) 0.25 M NaCH3CO2(aq), (c) 0.200 M CH3COOH(aq).

A: (a) 0.10 M NH4Cl(aq) The reaction is as follows,

Q: 3.1 9 (a) Define and write the expression of K for the dissociation of water W (H₂O). K is the W K =…

A: Dissociation of water:

Q: The molar solubility of europium (1) hydroxide is 1.37 x 10' M. What is the K value for the dsoation…

A: The equilibrium between the soluble ions and insoluble salt can be described by the solubility…

Q: Ksp for Agl = 1.2 x 10-17. Calculate the molar solubility of Agl in 1 x 104 molar AgNO3 solution.…

A: AgI⇌Ag+  + I-  let ,intial concentration of Ag+=x , I- =xIn AgNO3 solutionAgNO3⇌Ag+  +NO3- 10-4 M…

Q: 3) Determine the molar solubility of chromium(I) hydroxide in a buffered solution with pH = 11.45.…

A: Given: Kf of Cr(OH)3=3×1029 Ksp of Cr(OH)4-=8×10-29 pH=11.45

Q: NH4

A: Given: Ammonia buffer solution: M1 =  0.25 M [NH4+] M2   = 0.22 M [NH3] pKa of NH4+ = 9.24

Q: Sulfuric acid (H2SO4) is a strong acid in aqueous solution, yet the pKa of sulfuric acid is 7.6 in…

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Q: Sodium sulfate is slowly added to a solution containing 0.0500 M Ca² (aq) and 0.0260 M Ag+ (aq).…

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Q: What is the molar solubility of PbI2 in 0.10 M Pb(NO3)2 (aq)? [Hint: to which ion concentration…

A: The solution to the given numerical is as follows:

Q: The Ksp of AgI is 8.5 × 10–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at…

A: The equation corresponding to the solubility product of AgI can be written by multiplying the…

Q: Metal sulfides are prepared by bubbling hydrogen sulfide gas, H,S, through an aqueous solution…

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Q: A volume of 500.0 ml. of 0.100 M NaOH is added to 525 mL of 0.250 M weak acid (K, = 4.44 x 10-5).…

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution. Using…

Q: What mass of AgBr will dissolve in 500.0 mL of 3.10 M NH3? Ksp for AgBr is 5.0 x 10-13. For the…

A: Answer: Since, Ag+ is forming complex with NH3 but Br- is not reacting with anyone, therefore…

Q: Calculate the Kp of the following compounds, given their molar solubilities. (а) СuS, 7.33 х 10 19 М…

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Q: Sodium sulfate is slowly added to a solution containing 0.0500 M Ca² +(aq) and 0.0210 M Ag+ (aq).…

A: Given that, Initial concentration, [Ca2+] = 0.0500 M [Ag+] = 0.0210 M  We have to calculate the…

Q: ter the solubility expression for Mg3(PO4)₂(s). sp =

A: The solubility product constant (Ksp) is a equilibrium constant for a solid substance dissolved in…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.