What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kai- 4.3 x 10-7; Ka2 = 4.8 x 10-11 O 1.4 O 3.88 O 2.80 O 3.84 O 10.12

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: The given data contains, Ka= 7.10×10-4 Concentration of HNO2 = 0.120 M

Q: What is the pH of a 0.40 M ammonia solution? Ka is 5.6 X 10-10 11.43 O 2.57 O 9.18 O 4.82

A: Ka = 5.6 x 10 —10

Q: Carbonic acid, H2COS is a diprotic acid with Ka1 = 4.3 x 10 7 and Ka2 = 5.6 x 10 11. What is the pH…

A: Answer

Q: A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC gH 70 4) was dissolved in enough…

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Q: Malonic acid (Ka1 = 1.42 x 10–3, Ka2 = 2.01 x 10–6) can exist as one of the 3 forms shown below.…

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Q: What is the pH of a 0.25 M solution of NH3? Kb = 1.8x105 O 2.67 O 11.33 O 9.07 O 4.93

A: Given valuues from  the question, Salt concentration = c= 0.25 M Kb =1.8×10--5 then,

Q: What is the concentration of a weak acid if its Ka = 3.7 x 10-7 and its pOH = 11.62?

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Q: What is the COH of an acidic solution with a pH of 2.77? O-0.44M 0.44M 7.0 x 10-7M O1.7 x 10-3M O…

A: For [OH-] concentration we first to find the value of pOH with the help of this equation pH + pOH =…

Q: Find the pH of 0.180 M NACN solution. For HCN, K = 4.9 x 10 10 O 8.57 O 2.72 O 5.03 O 11.28

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Q: What is the pH of a 0.00138 M hypochlorous acid (HClO) solution?  Ka = 3.5 * 10-8 Report your answer…

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Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with a pH of 3.58? O…

A: pH is defined as negative logarithm of hydrogen ions present in the solution.

Q: What is the pH of a 0.0040 M Sr(OH)2 solution? O 12.00 O 2.40 O 11.60 O 11.90 O 2.10

A: Strong acids or bases  are dissociated completely. so we can direct calculate its [H+] or  [OH-]…

Q: What is the pH of a 0.100 M solution of potassium hydrogen phthalate, KHC8H4O2? For phthalic acid,…

A: Given data : Potassium hydrogen  phthalate, (KHC8H4O2 ) is a phthalic acid. So, pKa = -log[Ka] Ka =…

Q: What is the pH of a 1.40*10^ -2 mol/L Ca(OH)2 solution? (NOTE: To determine the actual hydroxide…

A: Given : Concentration of Ca(OH)2 = 1.40 X 10-2 mol/L

Q: Determine [OH–], pOH and pH of a 0.41 M  aqueous solution of LiC3H5O3 (K b = 7.1×10-11). [OH–] =…

A:

Q: Calculate the pH of an aqueous solution of 0.70 M H3BO3 and 0.40 M H;BO3 Acid Formula Ka pKa HCOOH…

A: Henderson - Hasselbalch equation:

Q: What is the pH of a solution with [H*] = 1.0 x 104 M? 0 7 O -4 O 4 O 10

A: The pH of the solution is defined as negative logarithm of the molar concentration of H+ ions.…

Q: What is the Ka of cyanuric acid if a 0.030 M cyanuric acid aqueous solution has a pH of 4.15? O…

A:

Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

A:

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: Calculate the pH of a 0.100M solution of the weak base NH3. Kb of NH3 1.8×10. %3D 3)

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Q: Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.     Ka = 7.11*10^-3

A: Given: Concentration of H3PO4 = 0.400 M And Ka of H3PO4 = 7.11 × 10-3  NOTE: Since only the 1st Ka…

Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kal= 4.3 x 10-7; Ka2 = 4.8 x 10-11.…

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Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

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Q: What is the pH of IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: What is the pH of a 0.02M ammonia solution if its Kb va www H.O + NH, 0H + NH,. O 3.2 O 12.3 O 10.8…

A: NH3+H2O⇌OH-+NH4+ NH3=0.02 M Kb=1.8+10-5

Q: For HNO2, Ka = 4.6 x 10-4 and for HSO4-, Ka = 1.2 x 10-2. Which is the stronger acid?

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Q: Calculate the pH of a 1.3 M Ca(OH)2 aqueous solution. 14.4 O 13.9 O 13.6 O 14.1

A: Answer: 14.4

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

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Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa).   Kb for HCOO− = 5.9 × 10−11

A: Given :-  [HCOONa] = 0.31 M  Kb for HCOO- = 5.9 × 10−11  To calculate :-  pH of solution

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A:

Q: 5. A 0.15 g Ca(OH)2 (MM = 74.092 g/mol) is dissolved in enough water to make a 0.500 L solution.…

A: Given, The mass of Ca(OH)2=0.15 g. The molar mass of Ca(OH)2=74.092 g/mol The volume of the…

Q: What is the pH of a solution with an acid concentration of 9.4 x 10-2 M? O a) 2.97 O b) 1.03 Oc)…

A: Acid Concentration = [H30+] = 9.4* 10^-2 Using the formula pH = -log[H30+] pH = - log (9.4*10^-2) pH…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105) NH3 - NH4 + OH a 13.987 O b .013 O c…

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Q: Give the formula of the conjugate acid:(a) O²⁻(b) SO₄²⁻(c) H₂O

A: An acid is a substance that furnish H+ ions in solution. A base is a substance that accepts furnish…

Q: Malonic acid (Ka1 = 1.42 x 10–3, Ka2 = 2.01 x 10–6) can exist as one of the 3 forms shown below.…

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Q: 5. Which of the following is Lewis acid BF3 FeC12 AICI3 All of the above

A: According to the definition of lewis acid is that, Element,atom or ion having incomplete octet or…

Q: Calculate the pH of a 0.10 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

A:

Q: Calculate the pH of a of 0.100M KBRO solution. Ka for hypobromous acid, HBRO, is 2.0 x 10 6- 10.85…

A: Given: The concentration of the KBrO3 solution = 0.100 M The Ka for HBrO3 = 2.0 × 10-9 We have to…

Q: What is the pH of a 0.02M ammonia solution if its Kb value is 1.8*10^.5? H.O + NH, 2 OH + NH,. 3.2 O…

A: The value of Kb for the given weak base is = 1.8×10-5 The concentration of the base solution is =…

Q: Determine the pH of 0.25M CH3COONA solution. Kg of CH3COOH = 1.8×105 Select one: 10.08 O 9.08 O 4.90…

A: Sodium acetate is a salt of a weak acid, acetic acid, and strong base, sodium hydroxide. The salt of…

Q: What is the pH of a 0.04 M of the diprotic acid H2CO3 solution? Kal= 4.3 x 10-; Ka2 = 4.8 x 10-11. O…

A:

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Since the Ka1 of H2CO3 is >> Ka2 of H2CO3  Hence we can assume only the first dissociation of…

Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 × 10-5) O 4.94 O 12.03 O 1 1.05 O 8.02 O 2.09

A: Given,  Concentration of NH3 = [NH3] = 0.075 M  Base dissociation constant of NH3 = Kb = 1.75 x 10-5…

Q: What is the pH of a 0.2 M solution of sodium propionate C2H5COONA (salt) solution? (For propionic…

A: pH is the potential of the hydrogen atom, pH is a logarithmic function, it is found from the…

Q: What is the pH of an aqueous solution at 25.0 °C in which [OH ]is 0.0045 M? O 2.35 O -11.65 O 11.65…

A: Answer: option c) 11.65 is the pH of the solution.

Q: What is the pH of a 0.025 mol/L solution of methanoic acid K=1.8x10

A:

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the value…

A:

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.