Calculate the concentration of ions in the following saturated solutions: (a) [I] in AgI solution with [Ag*] = 9.1 × 10-9 M, (b) [Al³+] in Al(OH); solu- tion with [OH]= 2.9 × 10° M.

Q: What is the pH of a buffer prepared by combining .92 moles of a weak base B, with .59 moles of…

A:

Q: A volume of 500.0 mL of 0.130 M NaOH is added to 575 mL of 0.200 M weak acid (K, = 3.20 x 10-5).…

A: Buffer are solution which resist change in PH when acid Or base are added to it  Here We are…

Q: A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 Maqueous HBr. The solution that remains is…

A: The reactions taking place are, HBr first reacts with Zn(OH)2 to give zinc bromide. The excess HBr…

Q: If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic…

A:

Q: TION 2 B: Titration of a r d principle, when ase, what does

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Q: A student has a sea water sample which contains Ca 2+ ions . Describe briefly how he will determine…

A: The seawater is hard water and contains calcium and magnesium ions. These calcium ions can be…

Q: The titration of a weak monoprotic acid by NaOH is shown here. The optimal buffering capacity of…

A: The titration curve given is,

Q: Which of the following calcium salts should dissolve in a strong acid, such as HCl: Ca(OH)2, CaSO4,…

A: Calcium hydroxide is known as slaked lime. It is a base and on reaction with acid, it forms a salt.…

Q: What is the pH of a buffer containing .0721 M Na2SO4 (aq) and .117 M NaHSO4 (aq)?

A: pH  of acidic buffer, pH = pKa+log([conjugate base]/[acid]).  pH  of acidic buffer, pH =…

Q: Of the following solutions, which has the greatest buffer capacity (assuming 1 L of each)? O 0.050 M…

A: Buffer solutions resist tochange in pH  According to  Henderson pH of acidic buffer is     pH = pKa…

Q: If you put a pure copper penny in an aqueous solution of AgNO3, which of the following will happen?

A: On putting a pure copper penny in an aqueous solution of AgNO3, a reaction will occur.

Q: Which of the following salts would be more soluble in acidic solution than in neutral water? A.…

A: The dissolving capacity of any component in fix amount of liquid is referred as solubility and the…

Q: A volume of 500.0 mL of 0.130 M NaOH is added to 555 mL of 0.250 M weak acid (Ka = 3.04 × 10¬³).…

A: Formula: pH = pKa + log[salt]/[acid] pKa = -logKa Number of mmoles = Molarity x volume (mL)

Q: A 98-mL sample of 0.62 M HNO2 (Ka = 4.0 ´ 10–4) is titrated with 0.25 M NaOH. What is the pH of the…

A: Number of mmols = Molarity x volume (mL) Number of mmols of NaOH added = 0.25 x 30 = 7.5 mmol Number…

Q: A plot of pH vs volume of 0.05 M NaOH solution was obtained for titrating 0.4055 g of a dried solid…

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Q: A buffer solution is made that is 0.401 M in HCN and 0.401 M in KCN. If Ka for HCN is 4.00 x 10 0,…

A: A buffer solution is made of a weak acid ie. Hydrocyanic acid (HCN) and potassium cyanide (KCN). pH…

Q: A volume of 500.0 mL of 0.110 M NaOH is added to 525 mL of 0.250 M weak acid (Ka = 2.53 × 10-').…

A: Concentration of NaOH=0.11M  Volume of NaOH=500 mL  Volume of weak acid=525 mL  Concentration of…

Q: Which of the following will raise the pH of a weak acid HA in aqueous solution? 1. addition of HNO3…

A: (I) HNO3 is a strong acid and thus decreases the pH of the solution. Therefore, pH won’t increase on…

Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…

A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…

Q: Calculate the molar solubility of BaSO4 in a solution containing 1.0 M SO4 -2 ions

A: Given , BaSO4 [SO42-]= 1.0 M

Q: A solution of HClO4 was standardized by dissolving 0.4008 g of primary-standard-grade HgO in a…

A: From 1 mole of HgO 2 moles of OH- are released. And HClO4 gives 1 mole of H+. Number of moles of HgO…

Q: 6. Calculate the pH of the solution that results when0.093 g of Mg(OH)2 is mixed with 75.0 mL of…

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Q: A buffer solution is 0.451 M in NaH PO, and 0.270 M in Na HPO4. If K, for H,PO, is 6.2x10, what is…

A: Henderson-Hasselbalch equation:- pH = pKa + {log[conjugate base]/[weak acid]}

Q: What [Ag+] is required to reduce [CO3 2−] to 8.2 × 10–4 M by precipitation of Ag2CO3?

A: We know that, the solubility product of salt that do not dissociate completely in the solvent can be…

Q: 2. There is a phosphate buffer with 0.1 M of NaH2PO4 0.1 M of Na2HPO4. Calculate pH of buffer…

A: pH of a buffer solution can be calculated using H-H equation.

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 is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.160 mol of KBrO in…

A: For HBrO , pKa = -log Ka = -log ( 2.5 × 10⁻⁹ ) = 9 - log2.5 = 9 - 0.40 = 8.60 For buffer : pH = pKa…

Q: The pH value for 0.01 M potassium cyanide is 7x10-10 respectively -(when Kw & Ka are 1x10-14 & ---

A: Given: Kw=1×10-14Ka=7×10-10 KCN(potassium cyanide) is a salt of a strong base (KOH) and a weak acid…

Q: The concentration of ammonia (17.031 g/mol) can be determined through back titration. After addition…

A: We need to calculate the concentration in %w/v of ammonia.

Q: write the reactions of Zn, Fe, and Cu metals with HCl and H2SO4 acids.

A: Reactions of metals like zn, Fe, Cu with HCl and H2SO4.

Q: Fe(OH)2(s) + Pb(OH)3-(aq) ---> Fe(OH)3(s) + Pb(s) in basic solution

A:

Q: Calculate the pH of the following two buffer solutions: (a)2.0 MCH3COONa/2.0 M CH3COOH, (b) 0.20 M…

A: The pH of a acidic buffer can be calculated as follows: pH=pKa+logSaltAcidwhere Ka is the…

Q: A buffer solution is made that is 0.402 M in HF and 0.402 M in KF. If Ka for HF is 7.20 x 10-4 what…

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Q: A 25.0 mL solution of 0.100 M CH3-COOH is titrated with a 0.200 M NaOH solution. What is the pH…

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Q: what is the pH of this buffer solution?

A: Given :-  concentration of HNO2 = 0.309 M  concentration of NaNO2 = 0.340 M  Ka = 4.5 × 10-4  To…

Q: A buffer solution is made that is 0.301 M in H2SO3 and 0.301 M in KHSO3. (1) If K, for H2SO3 is…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: A weak base, B, has a Kp value of 5.3 x 10-4. What is the hydroxide ion concentration in a 0.050 M…

A: Given-> Kb = 5.3 × 10^-4  Concentration = 0.050 M

Q: Calculate the molar solubility of Ni(OH)2 when buffered atpH (a) 8.0, (b) 10.0, (c) 12.0.

A: In a balanced chemical reaction, the product of the equilibrium concentration of the ions of the…

Q: The pH of buffer solution that has Ka = 6.23 x 105 and 5a, = 3a, is: а. 4.43 b. 4.03 С. 4.38 d. 3.98…

A: pH = d.  3.98

Q: Which of the following will raise the pH of a weak acid HA in aqueous solution? I. addition of HNO3…

A: (I) HNO3 is a strong acid and thus decreases the pH of the solution. Therefore, pH won’t increase on…

Q: er soluble ions produced by the addition of Na2O2 and ex

A: The chemical reaction between Na2O2 and excess KOH is given below: Na2O2 + 2KOH → 2NaOH + 2KO.

Q: Calculate the concentration of ions in the following saturated solutions. (a) [I-] in AgI solution…

A: The solubility product constant, Ksp​, is the equilibrium constant for a solid substance dissolving…

Q: What is the pH of the buffer that results when 3,06 g of NagHPO, and 2.17 g of NaH,PO, are diluted…

A: Mass of Na2HPO4 = 3.06 g Mass of NaH2PO4 = 2.17 g Volume of buffer solution = 0.3 L Ka of H2PO4- =…

Q: A buffer solution is made that is 0.432 M in H₂CO, and 0.432 M in KHCO3. If Kal for H₂CO, is 4.20 x…

A:

Q: The titration of Na,Se with HCI has the following qualitative profile. pH E F V2 mL HCI (a) Identify…

A: Point A : Na2Se  Point B : Na2Se + NaHSe  Point C : NaHSe ( first equivalence point)

Q: A buffer solution is made that is 0.475 M in HNO2 and 0.475 M in KNO2. If Ka for HNO2 is 4.50 x 10…

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Q: Explain the qualitative analysis of group 2 cations

A: Dilute HCl is added to the mixture containing cations. If it dissolves completely, group 1 is…

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.