Find the pH of the solution containing 0.04 M Na3PO4. (Ka1 = 7x10-3, Ka1 = 2.2x10-7, Ka3 = 4.5x10-13) Note: Write the relevant equilibrium reaction, state the equilibrium constant.

Q: Calculate the molar concentration of Agtao) kons in a 2.12 M solution of AgCl 2 with no excess…

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Q: Calculate the pH of a solution containing 0.0460 M potassium hydrogen tartrate and 0.028 M…

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Q: A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH. What volume KOH…

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Q: acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an…

A: Dissociation of weak acid: CH3COOH⇋CH3COO- + H+ Ka=CH3COO-H+CH3COOH

Q: In titrating 10 ml of 0.1 N HA (pKa-4),the pH after the addition of 12 ml 0.1N NaOH is O 3.69 О 11.2…

A: Given Normality of HA = 0.1 N Volume of HA = 10 mL Mole of HA = Normality of HA * Volume of HA Mole…

Q: 1. A natural lake has a pH of 5.2. In descending order of concentration (highest to lowest), the…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: 1) Use systematic treatment of equilibrium to find the concentrations of Mg2t, F, and HF in a…

A: We have find out the concentration of Mg2+,F- and HF in saturated solution of MgF2.

Q: Calculate the volume, in milliliters, of 0.170 M NAOH that must be added to 315 mL 0.0547 M…

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Q: Describe how you would accurately prepare 100.0 mL of a buffer solution with pH 4.7 using 1.0 M…

A: Given:  pH = 4.7  Ka = 1.8 x 10-5  pKa = -log(1.8 x 10-5) = 4.745  [CH3COOH] = 1 M  [NaOH] = 1 M…

Q: Solve for the pH level of an ammonia buffer. Given that it contains 500.0 mL of 0.3701 M ammonia and…

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Q: 2. Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99…

A: 2. Solution - According to the question - Given - 1. At 25 °C 2H₂O ⇌ H₃O⁺ + OH⁻ pH = ½pKw = ½ ×…

Q: a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of…

A: pH = 7 + (pKa + log C)/2 pOH = pKb + log [salt]/[base] pH + pOH = 14

Q: Just fill out Table 1 by writing “+” if the compound is soluble/miscible in the solvent. Otherwise,…

A: "Like dissolves like" is the thumb rule for dissolution of solute in solvent. This means highly…

Q: Prepare 500 mL of 0.1 M bicarbonate buffer solution, pH = 6, from 0.1 M stock solutions of carbonic…

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Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 409 mL 0.0463 M…

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Q: 3. 2.0-g NaF 6H2O is dissolved in enough analytical water to make 250.0- equilibrium concentration…

A: Sodium fluoride is a strong electrolyte and it is formed by the strong base, NaOH, and weak acid HF.…

Q: Both functional groups of salicylic acid ionize in water, with Ka = 1.0 × 10^-3 for -CO2H group and…

A: Given: Ka for –CO2H group = 1.0 x 10-3 Ka for –OH group     = 4.2 x 10-13 Solubility of salicylic…

Q: Use the pC-pH diagram for open carbonate system to find the equilibrium pH for a solution prepared…

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Q: 1. Predict if an aqueous solution of 0.5 M sodium cyanide, NaCN, would be acidic, neutral, or basic…

A: Hydrolysis is a reverse process of neutralisation, that is, in hydrolysis a given salt reacts with…

Q: Determine the pH during the titration of 39.6 mL of 0.226 M trimethylamine ((CH3)3N, Kp = 6.3x10-5)…

A: Since you have asked a question with multiples of parts we will answer only 1st 3 subparts for you.…

Q: calculate the pH of a solution that is 1.00 M CH3COOH (ka = 1.0 x 10^-5) and 1.00 M CH3COONa

A: Given: Concentration of weak acid CH3COOH = 1.00 M And the concentration of CH3COONa = 1.00 M

Q: When 10 drops of  0.1 M Co2+ is acidified using 20 drops 6.0 M CH3COOH and a pinch of solid NaNO2 is…

A: Co2+(aq) is oxidized in acidic medium(H+) in presence of NaNO2(aq) to form the yellowish-orange…

Q: Calculate the pH of a solution that is 0.200M in NH3 and 0.300M in NH4Cl. The dissociation constant…

A: Given: Concentration of NH3 = 0.20 M Concentration of NH4Cl = 0.30 M Kb = 1.75x10-5

Q: In the titration of 20 mL CH3COOH (Ka = 1.76 x 10-5) 0.4 M with a solution of NaOH 0.4 M, calculate…

A: The buffer is the solution of reagent that is used to maintain its pH (potential of hydrogen) when…

Q: Calculate the concentration of the carbonate and bicarbonate ion in one sample. (Ka2 H2CO3 is 4.7 x…

A: Molarity is concentration of substance in solution. pH help us to calculate hydrogen and hydroxide…

Q: Use the Henderson-Hasselbalch equation to calculatealculate the pH of the solution prepared by…

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Q: Calculate the pH when 1.77 g of C6H5COONa (FW = 144.1 g/mol) is added to 48 mL of 0.50 M benzoic…

A: Ka = 6.5 x 10-5 pKa = - log Ka = - log (6.5 x 10-5) = 4.187

Q: What is the pH of a solution containing 0.30 M lactic acid (K₂ = 1.38 x 10-4) and 0.50 M of lactate…

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Q: Calculate the pH of a solution containing 0.03 M NaH2VO4 and 0.05 M Na2HVO4. (Ka1 = 1.11×10-2, Ka2 =…

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Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

A: Given data, Ka for NH4+=2.0×10-5Kf for [Ni(H2O)5(NH3)]2+=501

Q: Calculate the pH of an acetic acid solution (initial concentration 0.01 M, Ka = 1.8 x 10-5) and the…

A: i) CH3COOH dissociates as follows:                  CH3COOH⇋CH3COO-+H+Initial               0.01…

Q: Calculate the equilibrium concentration of Ni²* in a solution with an analytical NİY2- concentration…

A: The metal complex equilibria value suggests that Y here is EDTA.

Q: Calculate the pH at intervals of 20mL (from 0 to 100 mL) by titrating 40 mL of hydrogencyanate (pKa1…

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Q: Calculate the degree of dissociation of .4 0.10 m acetic acid solution, Ka= 1.5 x 10-2 * ?that exist…

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Q: A chemist adds enough of the theoretical ionic compound MX3 to form a saturated solution. She knows…

A: One mole of MX3 will dissociates into 1 mole of M3+ and 3 mol X-. Let the solubility of MX3 be “s”

Q: Predict if an aqueous solution of 0.5 M sodium cyanide, NaCN, would be acidic, neutral, or basic at…

A: The questions are based on the concept of equilibrium. we have been given sodium cyanide which is…

Q: 8) 10.0 ml of.15M H3A (Kat = 2.5 x 104, Ka2 = 3.5 x 108, Ka3 = 5.0 x 10-12) is titrated with .10M…

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Q: Describe the preparation of 500 mL of 1.25 M phosphate buffer with pH of 6.75 using Solids:…

A: The Henderson-Hasselbalch equation gives a relationship between the pH of acids and their acid…

Q: for a weak HA acid with concentration 0.04 M and Ka = 4 × 10-⁹, find: a) the degree of dissociation…

A: Given [HA] = 0.04 M Ka = 4 × 10-9 pka = - log (Ka)          = - log( 4 × 10-9)          =  8.40…

Q: In titrating 10 ml of 0.1 N HA (pKa-D4),the pH after the addition of 12 ml C NAOH is O 3.69 O 11.2 O…

A: In this question HA is limiting reagent so NaOH and salt remains in the final solution.

Q: What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise…

A: The concentration of H2Se is 0.100 M. The dissociation constants, Ka1 and Ka2, of H2Se are 1.3×10-4…

Q: Calculate the concentration of the carbonate and bicarbonate ion in one sample. (Ka2 H2CO3 is 4.7 x…

A:

Q: Show how to prepare a 100-mL phosphate buffer solution (0.1 M, pH 7.0) using 14.8-M concentrated…

A: Given, Volume of buffer solution = 100mL = 0.2 L Molarity of buffer solution = 0.1M Molarity of…

Q: Calculate eq. concentrations when for 0.55 M HAc solution where ka(25C)=1.8x10^-5 with an ICE table.…

A: Look out this reaction as: HAc: concentration of acetic acid. H+: concentration of proton. Ac-:…

Q: Calculate the pH of a solution that is 0.553 M nitrous acid (HNO2) and 0.663 M of potassium nitrite…

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Q: What is the equivalence point volume of 0.140 M NAOH required to neutralize 75.0 mL of 0.350 M HC1?…

A: Concentration of NaOH=0.14M  Volume=75mL Concentration of HCl=0.35M

Q: What is the value of Q when the solution contains 2.00 x 10¬³M Ca2+ and 3.00 x 10-² M SO4²-?

A: To find Q?

Q: Find the pH and fraction of dissociation (a) of a 0.100 M solution of the weak acid HA with Ka =…

A: Given that, Ka of HA = 1.00×10-5  [HA] = 0.100M  Then,

Environmental Pollution

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