The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). Calculate the pH of a saturated solution of Mg3(AsO4)2 in water.

The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). Calculate the pH of a saturated solution of Mg3(AsO4)2 in water.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 75GQ

See similar textbooks

Related questions

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

Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…

A: Given that, Mass of formic acid = 0.3654 g Molecular mass of formic acid = 46.03 g/mol Volume of…

Q: 5.)Shortly after the dissolution of lead(IV) oxide, the dissolved Pb will react with water to form…

A: EPA is the Environmental Protection act. For environmental and sustainable welfare under EPA limits…

Q: Buffers that are based on 3-morpholinopropanesulfonicacid (MOPS) are often used in RNA analysis. The…

A: The pH range of the buffer solution is 6.5 to 7.9 The pKa value gives us the idea of the acidic…

Q: A 200.00 mL solution of 0.00105 M AB4 is added to a 270.00 mL solution of 0.00245 M CD5. What is…

A: Assuming the salts AB4 and CD5 are soluble in water completely as no information is given about…

Q: What would be the sulfide-ion formality in a saturated solution of Bi2S3 if the Ksp of this…

A: Bi2S3======> 2Bi ³+ + 3 S²- Suppose, “x” is the Solubility of Bismuth Sulphide....

Q: Calculate the pH of a solution saturated in calcite and in equilibrium with atmospheric CO2. The…

A: The Ksp expression for the solubility of CaCO3 can be expressed as: Ksp=Ca2+CO32-…

Q: Your research advisor asks you to prepare a buffer solution at pH = 12.5 with capacity of about…

A: To make a buffer of desired pH/pOH with best buffer capacity, that acid /base should be used which…

Q: Given that the molar solubility of Pb(IO3)2 in a 0.100 M solution of NaIO3 is 2.4 × 10–11 M,…

Q: Properties of a Buffer The amino acid glycine is often used as the main ingredient of a buffer in…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW = 53.491 g/mol). Kb = 1.8…

A: First we would Calculate initial pH of solution before adding HCl. Then pH after adding HCl is…

Q: Solve the following problem: Calamine, which is used to relieve skin irritations, is a mixture of…

A: The balanced equation for the reaction of Zn2+ with EDTA(Y4-) is: Zn2+ + Y4- -----> ZnY2- Mole…

Q: 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: The following observations are made about a diprotic acidH2A: (i) A 0.10 M solution of H2A has pH =…

Q: The Ksp for nickel(II) hydroxide at 25 degrees Celsius is 2.0 * 10^-14. What is the molar solubility…

A: Given that: Solubility product constant (Ksp) of Ni(OH)2 = 2.0×10-14 pH = 10.102 At 25°C pH + pOH =…

Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 will be respectively equal…

A: pKb = - log Kb = - log ( 1.8 x 10-5) = 5 - 0.26 = 4.74 C = 0.1 N For salt NH4Cl pH = 0.5 (pKw - pKb…

Q: 120 mg of codeine hydrochloride (CodHCl) is dissolved in 10.0 mL of water. Calculate the expected…

A: Since you have posted multiple completely unrelated questions, we are entitled to answer the first…

Q: The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKp of this…

Q: Calculate the weight of solid sodium formate (HCOONA: MW = 52) that should be dissolved in 1-L of…

A: PH of a buffer, pH=pKa+log (sodium formate/formic acid) Given ka=1.7×10^-4 Pka=-log 1.7×10^-4 =3.77

Q: a. Calculation of the pH of a Solution of a Polyprotic Acid Histidine has ionizable groups with pKa…

Q: The molar solubility of sulfathiazole (weak acid) in water is about 0.001 M. a. What is the lowest…

A: Given: pKa of sulfathiazole = 7.2 Molar solubility of sulfathiazole = 0.001 M

Q: If K-2.35 & K,- 1.32 x 1010 Suppose 50ml of 0.010M aqueous amine is extracted with 100ml of benzene.…

A: Given: K = 2.35 Ka=1.32×10-10 Volume of aqueous amine = 50 mL Volume of benzene = 100 mL…

Q: 5. Magnesium hydroxide (Mg(OH)2) has a pKsp value of 11.25. In a solution at pH 10, what is the…

A: Given, pKsp of Mg(OH)2 = 11.25 pH = 10 What is the maximum Mg2+ concentration in µmol/L = ? What…

Q: A saturated aqueous solution of Ni(OH)2 has a pH of 11.8. Calculate the Ksp of the solution and…

Q: Using the concentrations 0.100M and 0.1766M, and the pKa of 3.752, what is the theoretical pH of a…

A: pKa = 3.752

Q: The solubility of CO2(g) in water at 25 °C and under a pressure of 1.00 atm is 1.45 g/L. If the air…

A: Air pressure is 1.00 atm. Pressure of CO2 in air =0.036100×1.00 atm=3.6×10-4 atm

Q: Consider an amphoteric hydroxide, M(OH), (s), where M is a generic metal. M(OH), (s) = M²+(aq) + 2…

A: The reaction is as follows: M(OH)2(s)⇌M2+(aq)+2OH-(aq) 1) Calculation of concentration of OH- at pH…

Q: A sample of water at pH 10.5 has 75 mg/L of CO3-2 and 65 mg/L of HCO3- Including the contribution of…

Q: Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several…

A: Answer -

Q: What is the pH of an acidic mixture containing 0.062 M hydrazoic acid (Ka = 1.9 * 10-5) and 0.062 M…

A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…

Q: If a saturated solution prepared by dissolving Ag2CO3 in water has [Ag*] = 2.56 × 10 M, what is the…

A: Given [Ag+] =2.56×10-4 MFind outKSP for Ag2CO3=?

Q: 2) The above weak base, BOH having K, of 1.8x10 is required to transform into a Buffer solution. The…

Q: The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4…

Q: Prepare 250ml of the following buffer solutions. Concentration Buffer solution pka Desired ph…

A: Since you have asked multiple questions with multiple subparts, we will answer first three subparts…

Q: How many grams of dipotassium succinate trihydrate (K2C4H4O4-3H2O, MW = 248.32 g/mol) must be added…

A: Given, The pH of the solution is 5.813. The molarity of succinic acid is 0.0338 M. pKa2 is 5.636.…

Q: Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His = imidazole…

A: The three pKa values shows that there are 3 replaceable hydrogens in the molecule(represented as…

Q: If the Ksp for PbSO, is 1.7x10-8 , calculate the SO,2- in PBSO4 saturated solution.

A: Solubility product is the mathematical relation product of dissolved ion concentration which raised…

Q: The ionization constant (Ka ) equation of a monoportic weak, HA, acid is given by ca2 K = (1-0) The…

A: The solution is given below -

Q: Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of…

A: The pH for the solution of 2.00 M Na2CO3 is to be calculated. Given: pKa1 = 6.37 pKa2 = 10.32.…

Q: Commercial phosphate buffers are sold to maintain fish tanks at a pH of 7. Use a table of acid…

A: Acid dissociation equilibrium constants for H3PO4 are : Ka1 = 7.2 x 10-3 Ka2 = 6.8 x 10-8 Ka3 =…

Q: The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4…

A: (a) Mola solubility of Mg3(AsO4)2 in water; Ksp for Mg3(AsO4)2 =2.1 x 1020. Mg3(AsO4)2 ⇋ 3Mg2+…

Q: Consider the following: HClO2 + NaOH => H2O + NaClO2 50.0 mL of 0.250 M chlorous acid (HClO2,…

A: The balanced neutralization reaction is: HClO2(aq) + NaOH(aq) → NaClO2(aq) + H2O(l) Since all the…

Q: Sketch a titration curve for the amino acid cysteine, and indicate the pKa values for all titratable…

A: Cysteine is a polar uncharged amino acid containing a thiol group (SH), which on reaction with thiol…

Q: Calculate the molar solubility of BaCO3in a 0.10 M solution of Na2CO3(aq). (Ksp(BaCO3) = 8.1 x 10-9)

A: The given reaction of BaCO3 - Now calculate the molar solubility of BaCO3 -

Q: 11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5…

Q: To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should…

A: Henderson-Hasselbach equation. this equation shows the relationship between pH of a solution, the…

Q: Ksp for Agl = 1.2 x 10-17. Calculate the molar solubility of Agl in 1 x 10-4 molar AGNO3 solution. O…

A: The given data contains, Ksp for AgI=1.2×10-17Ag+=1×10-4 M.

Q: What is the pH of a saturated solution of sodium carbonate? (Solubility in water is 21.6g/100ml at…

A: Given , Solution of sodium carbonate. Ka1=4.5×10-7Ka2=4.7×10-11 Solubility in water = 21.6 g/ 100…

Q: Calculate the pK, of hypobromous acid from its K, value.

A: Since you have posted multiple questions, we are entitled to answer the first only.

Question

The value of Ksp for Mg₃(AsO₄)₂ is 2.1 * 10^-20. The AsO₄^3- ion is derived from the weak acid H₃AsO₄ (p_Ka1 = 2.22; p_Ka2 = 6.98; p_Ka3 = 11.50). Calculate the pH of a saturated solution of Mg₃(AsO₄)₂ in water.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Step 8

Trending now

This is a popular solution!

Step by step

Solved in 8 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A weak acid, HA, has a pKa = 6.2. If a solution of NaA(aq) is prepared, what does the pH of the solution need to be adjusted to in order to achieve the following ratios of deprotonated to protonated species? 1) [A-] / [HA] = 0.01 2) [A-] / [HA] = 10 3) [A-] / [HA] = 1 4) [A-] / [HA] = 106 Note: NaA is the sodium salt of , the conjugate base of HA. Assume NaA completely dissociates in water.
(b) Calculate the pH of 0.0005 mol dm-3 ethanoic acid when its pKa = 4.75 and explain the assumptions made in the calculations CH3COOH(aq)  CH3COO-(aq) + H+(aq) Ka = pH =
Consider the following expression for the equilibrium constant that represents the dissociation of iodic acid into hydronium and iodate ions. Ka [H3O+] [103] [HIO3] = = 0.161 When 176 g of iodic acid is dissolved in water to give an aqueous solution with a final volume of 1.00 L. Calculate the % dissociation of iodic acid to form iodate anions. The molar mass of iodic acid is 175.91 g mol-¹. a. 0.161% b.16.1% OC. 32.8% Od. 40.1% e. 83.9%
A buffer solution is 0.371 M in NaHS03 and 0.399 M in Na2S03. If Ka for HS03-is 6.4 × 10-8, what is the pH of this buffer solution? The pKa value for HSO3 is 7.19. What mole ratio of Na2SO3 to NaHSOs is needed to prepare a buffer with a pH of 6.97? [s032] [HS03-]
Calculate the pH at25°C of a 0.37M solution of sodium propionate NaC2H5CO2. Note that propionic acid HC2H5CO2 is a weak acid with a pKa of 4.89.
Find the pH and the concentrations of H2SO3, HSO3, and SO23 in each of the following solutions: (a) 0.050 M H2SO3; (b) 0.050 M NaHSO3; (c) 0.050 M Na2SO3.
From the reaction CaCO3+CO2+H2O= Ca2+ + 2HCO3- A.) Show how it affects the chemistry of water, alkalinity and hardness of water B.) Its relationship to microbial degradation of organic matter
What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the Kp for CH3NH2 is 4.4 x 104 and the Ka for HNO3 is 2.4.
Phosphoric acid (H₃PO₄) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70?
Phosphoric acid (H₃PO₄) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70? Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH of a 0.62 M solution of carbonic acid? A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution of H₂A? What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in 2.0 L of solution?
Phosphoric acid (H3PO4) is a triprotic acid with pKa values of 2.12, 7.21, and 12.32. It is a useful buffer solution for pH values near the pKa values. You have a 0.100 M solution of phosphate buffer with a pH of 2.50. How many mL of 0.500 M NaOH solution must be added to 1.00 L of this buffer solution to convert it to a buffer at pH 7.70? Answer in mL
Hydrogen peroxide (H2O2) can also form as a by-product during free radical oxidation reactions. H2O2 possesses a pKa value of 11.6. Based on this information, calculate the pH of a 1.80 L aqueous solution if 28 g of H2O2 is formed in a reaction.