Calculate the concentrations of H2SO3 and HSO3− in a 0.510 MM solution of H2SO3 Ka1=1.6×10−2 and Ka2=6.4×10−8).

Q: The hydronium ion concentration of an aqueous solution of 0.402 M hypochlorous acid (Ka = 3.50×10-8)…

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Q: What is the concentration of a solution of (a) KOH for whichthe pH is 11.89, (b) Ca(OH)2 for which…

A: We know that, the pH of the solution is equal to the negative log10 of the hydrogen ion…

Q: Determine the pH and equilibrium concentrations of all species of a 25 M H2SO3 solution at 25oC

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Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.630 M? (Kb = 1.3…

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Q: Calculate the volume of 0.230-M NaOH solution needed to completely neutralize 64.1 mL of a 0.850-M…

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Q: A theoretical compound B3(OH)2 is a strong base that has a pH of 13.51. Determine the concentration…

A: The given data is as follows: The pH pf B3OH2 solution = 13.51 The concentration in molarity = ? The…

Q: 11. What volume of 0.115 M HCl solution is needed to prepare 350.0 mL of a solution of HCl with pH…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pH of a 0.083 M solution of NaCN?

A: Given :- Concentration NaCN solution = 0.083 M  To calculate :- pH of solution

Q: 7. At 25°C, an aqueous solution of AlBr3 will have: (a) pH >7 (b) pH = 7 %3D (c) pH < 7

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Q: Calculate the molar concentration of OH− ions in a 0.069 M solution of ethylamine (C2H5NH2;…

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Q: A 1.00 L solution contains propanoic acid (C3 H5 O2 H) with a concentration of 0.350 mol/L, and…

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Q: Which of the following salts give acidic aqueous solutions? (1) KNO3 (2) KCH3COO (3) NH4NO3 (4)…

A: Strong acid + strong base = neutral Strong acid + weak base = acidic solution Weak acid + strong…

Q: Determine the pH of a 0.65 M solution of HCO₂K. The value of Ka for HCOOH is 1.8 × 10⁻⁴.

A: HCOOK is a salt of a weak acid (HCOOH) and a strong base (KOH). The salt is present as HCOO- and K+…

Q: What is the pH of a solution that is 0.400 M in NH3 and 1.450 M NH4*? Ka= 5.7x1010

A: Given :-  Concentration of NH3 = 0.400 M  Concentration of NH4+ = 1.450 M  Ka = 5.7 × 10-10  To…

Q: Calculate the OH- ion concentration of a 6.2 x 10^-3 M HClO3 solution

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Q: A solution of 0.05 M in NH4CI and 0.03M in NH3, calculate its OH- concentration and its pH. (pKa…

A: Concentration of NH4+ = [NH4+] = 0.05 M Concentration of NH3 = [NH3] = 0.03 M OH- concentration of…

Q: What is the concentration of ion or molecule in the solution of 0.0150 M C6H12O6?

A: Given: 0.0150M C6H12O6The given molar solution contains molecules of C6H12O6 since no ions are…

Q: What is the pH of a solution of 0.010 M CH3NH3ClO3?

A: Given that:  [CH3NH3ClO3] = 0.010M CH3NH3ClO3 is salt made up of weak base methyl amine(CH3NH2) and…

Q: What is the pH of a 0.258M solution of NaIO3?

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Q: A 0.050 M concentration of weak base, CH​3CH​2NH​2, was found to ionize at 1.7%. What is the…

A: Ethylamine (CH3CH2NH2) is a weak base. When diluted with water, it partially ionizes producing…

Q: 4. Calculate the pH of an aqueous solution containing 6.32x109 H3O* ions per liter.

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Q: Calculate the pH of 0.02354 M CH3 CO2 H and 0.1702 M NaCH3 C02. {Ka = 1.8 x10 °}

A: Given: [CH3CO2H]=0.02354 M [NaCH3CO2]=0.1702 M pH=? Ka=1.8 x 10-5

Q: Calculate the PH of:     II. A "1.8x10-2 molar" solution of an unknown strong base: X (OH) 2

A: Bases have Hydroxide ions(OH-) pH + POH = 14 POH = - log [OH-]

Q: What mass of NaOH(s) must be added to 1.0 L of 0.045 M NH3 to ensure that the percent ionization of…

A: The reaction happening is as follow:                           NH3 + H2O ----&gt; NH4OH…

Q: Write the equations for the dissocation of the following in aqueous solution:Na2S:[(NH4)2]CO3:KHSO3:

A: A compound dissociates into its corresponding ions in aqueous solution.a) Sodium sulphide…

Q: 6. Calculate the pH of the solution if the concentration of [H3O] ion is 2.0x10 M at 25°C.

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Q: What is the total molar concentration of ions in 0.750M solution of K2CO3 assuming complete [3]…

A: Molarity: In chemistry, the strength of solutions i.e. the number of ions of the solute per unit…

Q: Which correctly shows the ionization of H2CrO4 in water?

A: The acid given is H2CrO4.

Q: Calculate the pH of a 0.633 M NH, solution. NH, has a Kp 1.8 x 10–5.

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Q: Determine the hydroxide ion concentration in an aqueous solution of HBr with pH = 3.98 at 25 °C.…

A: Given: pH= 3.98 As we know, pH= -log[H+] So, [H+]= 10-pH  [H+]= 10-3.98  [H+]= 1.04 ×10-4M…

Q: What is the concentration of sodium ions in 0.105M Na2HPO4?

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Q: 7.8 Write equations to illustrate the amphoteric behaviour of [HCO3]¯ in aqueous solution.

A: Given, Amphoteric behavior of  [HCO3]- in aqueous solution     Required,…

Q: 4. Explain both HCO3¯ and HSO4¯ act as amphoteric substance.

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Q: Carbonic acid, H,CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 x 10-1". What is the pH…

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Q: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…

A: Given,  for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…

Q: Calculate the concentration of CO32- in an aqueous solution of 2.23x10-2 M carbonic acid, H2CO3…

A: Given,  Concentration of aq. carbonic acid, [H2CO3] = 2.23x10-2 M

Q: The hydronium ion concentration of an aqueous solution of 0.428 M hypochlorous acid (Ka = 3.50×10-8)…

A: In given question acid is weak like as CH3COOH that's why Ka is given  So use formula for Weak acid…

Q: Which of these aqueous solutions is expected to have the highest pH at 25 °C? 0 1.0 М Са(ОН)2 0 1.50…

A: pH of Acid is below 7 and pH of base is above 7.

Q: In a 0.080 M NH3 solution, what percent of the NH3 is present as NH4+?

A: The equation for the reaction is:

Q: If it takes 88 mL of 5.4 M KOH to neutralize 210 mL of sulfuric acid (H2SO4) solution, what is the…

A: The equivalence point is defined as the point in reaction when moles of acid equals the mole of base…

Q: at room temperature, calculate solutions of (i) KNO 3, (ii) CaC

A: The solution of given as,

Q: What is the pH of a solution with [H3O*] = 3.2x10-5M H3O*?

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Q: The hydronium ion concentration of an aqueous solution of 0.325 M nitrous acid (Ka = 4.50×10-4) is…

A: Given that -  Molarity of nitrous acid, HNO2 = 0.325 M  Acid dissociation constant, Ka = 4.50×10-4…

Q: Write an equation for the neutralization reaction of aqueous HBr and aqueous Ba1OH22.

A: An acid and a base react to form a salt and water.  HBr is an acid . Ba(OH)2 is a base.

Q: What concentration of KNO2 must be added, at 25 degrees Celsius, to 0.50 M HNO2 to result in a…

A: The solution mixture is a buffer solution of weak acid HNO2 and conjugate base NO2- ( as KNO2…

Q: Indicate the ionic species of ammonia that predominates at pH 4, 8, and 11.

A: Given: The ionic species of ammonia that predominates at pH 4, 8, and 11.

Q: Calculate the pH of a solution with a H3O+ concentration of 5.8 × 10^-4 M

A: Given: Concentration of H3O+ = 5.8*10-4 M

Q: What is the concentration of H3O+ in an aqueous solution with pH of 8.2?

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Q: actual concentration of the molecular form of HF

A: