Aqueous solutions of aluminum ions Al^3+ are acidic while those of carbonate CO3^-2 are basic why?

Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?

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Q: Calculate the pH of a 0.381 M NH, solution. NH, has a Kp = 1.8 x 10-.

A: pH: The negative logarithm of H+ ion concentration is known as pH. Ammonia in water behaves as a…

Q: What is the equilibrium constant of the HSO4-ion, if [H3O+] = 0.027 M; [HSO−4] =0.29 M; and [SO2−4]…

A: The Complete and balanced chemical equation is given as,

Q: Calculate the pH of a 0.043 M NaF solution. (K, for HF = 7.1 x 104.)

A: Given -> Molarity of NaF = 0.043 M Ka ( HF) = 7.1 × 10^ -4

Q: Calculate the pH of a 0.053 M NaF solution. (Ka for HF = 7.1 x 10−4.)

A: NaF is a salt of strong base (NaOH) and weak acid (HF)

Q: Estimate the pH of a 0.016 aqueous lead(ll) chloride

A: Hydrolysis of PbCl2 can form a weak base, Pb (OH) 2 and Cl- that does not combine with H+ as HCl is…

Q: The pH of a 0.12 M HNO3 solution is -1.22 -0.92 0.92 1.22

A: Given concentration of HNO3 = 0.12 M

Q: Write a net ionic equation to represent the reaction of (a) aqueous strontium hydroxide with nitric…

A: A net ionic equation for the reaction of strontium hydroxide with nitric acid has to be written.

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…

A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid

Q: Calculate the pH of a solution that is 0.410 M in HOCI and 0.050 M in NaOCI. [Ka(HOCI) = 3.2 x 10-8)…

A: Concentration of HOCl=0.410M Concentration of NaOCl=0.050M Ka(HOCl)=3.2 × 10^-8

Q: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca1OH22?

A: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca(OH)2?

Q: Calculate the pH of a solution containing 0.3 M HCOOH and 0.1 M HCOO (pKa of HCOOH = 3.76)

A: Concentration of HCOOH (Acid) = 0.3 M  Concentration of HCOO- (conjugate base of acid) =  0.1 M  pKa…

Q: er the following solutions are acidic, basic, or nearly neutral: (a) NaBr, (b) K2SO3, (c) NH,NO2,…

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Q: What is the hydronium ion concentration of a solution at 25C with a pOH of 4.7?

A: pH+pOH = 14 pH = -log[H3O+]

Q: Irite the balanced net ionic equation for H,SO4 reacting with Mg(OH)2. Remember to include phase…

A: Applying concept of ionic equation determination.

Q: Oxides can react with water to form acids or bases. Identify each of the following oxides as acidic…

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Q: 9 Write the formula of the conjugate acid of a HSO, b CO;?

A: According to Bronsted Lowry Theory , any molecule that donate H+ atom is an acid and any molecule…

Q: The acid ionization constant for Fe(H20)63+(aq) is 7.7×103. Calculate the pH of a 0.2920M solution…

A: The PH can be calculated as follows

Q: The pH of a 0.10 M solution of Ni(NO3)2 is 5.0. Calculate the acid ionization constant of Ni(H 2O)…

A: [Ni(H2O)6]2+ is a Bronsted- Lowry acid. It releases H3O+ in solution.The acid ionization reaction is…

Q: Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17).

A: Molarity of Solution = 0.010M Ka of Acid = 0.17 We have to find the pH of the solution of iodic…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.140 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Given : Concentration of HNO2 = 0.300 M Concentration of NaNO2 = 0.140 M And Ka of HNO2 = 4.5 X 10-4…

Q: 2. You have a solution of 0.1M Na₂CO3. You measure the pH using a pH meter. What is your prediction…

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Q: What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4?

A: Given : Concentration of NaH2PO4 = 0.042 M Concentration of Na2HPO4 = 0.058 M

Q: Water with an alkalinity of 2.00 x 10-3 eq/L has a pH of 7.0. Calculate [CO2], [HCO3-], [CO32-], and…

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Q: 0.1 M NaHCO3 solution, using the given pH data, calculate value of (Ka or Kb)

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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: 1. Calculate pH and concentrations of the ions for ammonia aqueous solution with concentration 0.010…

A: Given that : The concentration of ammonia = 0.010 M The pKb of ammonia is 4.76. We have to calculate…

Q: 3. How is K, obtained by the half-neutralization method?

A: Since you have posted multiple questions, we will solve the first question. Please post rest of the…

Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

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Q: Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write…

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Q: Which of the following substances can be classified as a Lewis base? CO Cu F a) O, only b) O, and CO…

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Q: Five solutions A, B, C, D and E when tested with universal indicators showed pH as 4, 1, 11, 7 and 9…

A: Five solutions A, B, C, D and E when tested with universal indicators showed pH as 4, 1, 11, 7 and 9…

Q: Calculate the pH of a 0.37 M solution of sodium hydrogen sulfite,  (6.0x10^-8). pH =

A: The pH of a 0.37 M solution of sodium hydrogen sulfite is to be determined. (Ka = 6.0x10-8).

Q: Calculate the pH for a 4.3 × 10−8 M HCl solution with an ionic strength of m = 0.1. yH+ = 0.83, yOH−…

A: We have to Calculate the pH for a 4.3 × 10−8 M HCl solution

Q: Calculate the fluoride ion concentration and pH of a solution that is 0.20 M in HF and 0.10 M in…

A: Common Ion effect: It is defined as the effect in equilibrium that occurs when common ion is added…

Q: 22:b) Solution A has a PH = 8.94 and Solution B has a [OH] = 4.5 x 10+ M. Which solution is more…

A: Here is the solution

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: What is the pH of a 0.460 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: The following reaction has a AG° value of +8.43 kJ/mol at 25 °C. HA(aq) + H20(1) =H;0*(aq) +A (aq)…

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Q: What is the pH of a solution of 0.0745 M NACH3O2 ? Ka = 1.8 x 10

A: Given: Concentration of NaC2H3O2, [NaC2H3O2]= 0.0745M Ka = 1.8 x 10-5

Q: Briefly explain why Fe* is a Lewis acid, but Fe" is not a Brønsted-Lowry acid.

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Q: The K, for hypoiodite anion (IO) is 4.35x10-4. What is the pH of a 0.226 mol L solution of lithium…

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Q: A patient’s sputum was collected for a laboratory analysis. The results revealed that the [H3O+]…

A: Given data contains, The concentration of hydronium ion is 5.2 x 10-7 M.

Q: The hydrogen ion concentration of sulphuric acid is 0.01. Calculate its pH.

A: Given - Hydrogen ion concentration of sulphuric acid = 0.01 M

Q: Calculate the pH of a solution of 0.25M Nacio(ag). The Ka of HCIO is 2.9 x 108.

A: NaClO is a salt of weak acid HClO. It has pH greater than 7 as it is base.

Q: Calculate the pH of the solution produced when 20.0 mL of o.125 mL of each of the following: a.…

A: d) moles of HCl = 0.125×0.02 = 0.0025 mol Moles of HClO4 = 0.2 × 0.5 = 0.01mol Total moles of H+ =…

Q: What is the concentration of each ion in each of the following solutions? (assume complete…

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Q: Trisodium phosphate (Na3PO4) is available in hardware stores as TSP and is used as a cleaning agent.…

A: Calculation of no. of mol of Na3PO4: n=given massMolar mass=35.0 g163.94 g/mol=0.2135 mol…

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.