The ionic strength of 0.10 M AI(NO3)3 is: O 0.30 O 0.10 O 0.70 O 0.60 O 0.20

Q: What is the pH of a solution with [H3O+]=2.42 x 10-4?

A: pH of any solution is given by  pH = -log[H3O+] where [H3O+]= concentration of H3O+ ions

Q: What is the pH of a 0.0300 M solution of NaNO2? (K, for HNO2 = 4.00 x 104) %3D O 7.00 O 7.94 8.81…

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Q: Write down the reaction between [Cr(C2O4)2(H2O)2] and dilute potassium hydroxide.

A: The given compound must be [Cr(C2O4)2(H2O)2]- instead of [Cr(C2O4)2(H2O)2]. [Cr(C2O4)2(H2O)2]-…

Q: Calculate the pH of a 0.23 M sodium formate solution (HCOONA). Kp for HCOO = 5.9 x 10-11

A: Given that,    Concentration of HCOONa solution = 0.23 M   Kb for HCOO-  = 5.9×10-11  Since, pKb =…

Q: B) Write a mass balance for a solution of Al2(SO4)3 if the species are Al, Al(OH), Al(OH);,…

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Q: Express the concentration of a 5% w/v sulfuric acid (sp.gr. 1.80) in %wiw. O a. 2.78 %w/w O b. 1.77…

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Q: What is the pH of a solution with a fluoride concentration of 0.18 M ? The Kb for F– is 1.47×10-11 .

A: pH: It measures hydrogen ion concentration, which helps in a measure the acidity of the solution,…

Q: What is the activity coefficient of Hg22+ in a solution of 3.3 mM Hg2(NO3)2? O 0.67 O 0.65 O 0.63 O…

A: Given, Concentration of Hg2(NO3)2 is 3.3 mM activity of Hg22+ =  ?

Q: Calculate the ionic strength (j) for a) the solution of AlCl3 (0.01 N) + Ca(NO3)2 (0.002 M)…

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Q: the ionic strength of a 0.05F H3PO4

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Q: What is the thickness of the ionic atmosphere (in nanometer, nm) for a solution of 0 29 mol/L of KCP…

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Q: As2. .. What is the minimum pH needed to prepare 1% sodium phenobarbital in water? Intrinsic…

A: We have to prepare 1% sodium phenobarbital in water. Solubility = 0.004M MW = 232.2g/mol pKa = 7.41

Q: Calculate the ionic strength of 0.5M Al2(SO4)3.

A: Al2(SO4)3 ----> 2Al3+ + 3SO42- 0.5 M                1 M         1.5 M Ionic strngth = 1/2 ΣCiZi2…

Q: What is the ionic strength of a 3:2 electrolyte with a concentration of 0.100 M? O 1.5 M O 16 M O…

A: Solution is made up of two components: solute and Solvent. Component which is present in major…

Q: which of the following would be a the reaction of Ca o plus NaF

A: When calcium oxide reacts with sodium fluoride gives calcium fluoride and disodium oxide.

Q: Calculate the pH of a 0.65 M solution of aqueous bromous acid (HBrO2, Ka = 1.2 x 10-5).

A: Dissociation constant of acid (Ka) - In dissociation reaction of acid, ratio of concentration of…

Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 x 10-5) %3D O 4.94 O 2.09 11.05 O 12.03 8.02

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: The concentration of PO43 ions in (M) found in a solution of 3 M H3PO4 is (Ka1= 7.1X10-3, K,2=…

A: H3PO4 is a tribasic acid and it gives 3 protons on dissociation. These steps take place one by one.…

Q: Barium fluoride (BaF2) has Ksp = 1.8 x 107. VWhat is the maximum fluoride ion concentration possible…

A: Given: Ksp of BaF2 = 1.8 x 10-7 Concentration of Ba2+ = [Ba2+] = 5.0 x 10-4 M

Q: (Calculate the molar (M) concentration of H2S04 solution of 0.250 N, to produce sulphate ion S04^(-2…

A: Given concentration of H2SO4  = 0.250 N  where "N" indicated for Normality    We know that…

Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?

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Q: A. Calculate the PH of the (0. 1 N) NasPOa in 250 ml B. What is the Normality of a sulfuric acid…

A: (A) pH of 0.1N Na3PO4 solution: C = 0.1/3 = 0.033M PO43- ions are undergoing hydrolysis and pH is…

Q: The ionic strength of 0.10 M AI(NO3)3 is: O 0.10 O 0.70 O 0.30 O 0.20 O 0.60

A: Given,  Concentration (C) of Al(NO3)3 = 0.10 M  Find ionic strength of this solution  Options are :…

Q: Calculate the pH of a 0.500 M aqueous solution of NH3. The Kp of NH3 is 1.77 x 10-5 O 8.95 O 11.47 O…

A: Given: Molarity of aqueous solution of NH3 = 0.500 M Kb of NH3 = 1.77×10-5

Q: What is the molar ratio of Fe(III) ion (Fe3+) to [Fe(SCN)6]3−?

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Q: A 0.100 M solution of nitrous acid (HNO2) had a pH of 2.07. What is the Ka value for nitrous acid.…

A: We are given Nitrous acid and its pH. We have to find Ka. Concentration of nitrous acid = 0.1 M

Q: The acid ionization constant for Co(H 2O) 62+(aq) is 3 ×10-10. Calculate the pH of a 0.10 M solution…

A: In this complex  CoH2O6+2Co is present in +2 oxidation state . For this we have to use complete…

Q: Calculate the concentration of F- in equilibrium with 0.0034 M Ba2+.

A: Barium ion and fluoride ions combine to give barium fluoride. The knowledge of its solubility…

Q: mine the pH of a 0.52 M lithium nitrite solution. (Ka for nitrous acid = 4.5 x 10-4 7.00 12.18 8.53…

A: Given, the Ka for nitrous acid = 4.5×10-4 We have to calculate the pH of 0.52 M lithium nitrite…

Q: What is the pH of 0.035 mol L solution of HF (K, = 6.8×104)? %3D

A: In the question, we are given- Concentration of HF = 0.035 mol L-1 Ka = 6.8 x 10-4

Q: What is the pH of a solution with a fluoride concentration of 0.20 M ? The Kb for F– is 1.47×10-11 .

A: In order to find the pH of the solution we first write down the given data: Fluoride concentration=…

Q: What is the pH of a solution with a fluoride concentration of 0.11 M ? The Kb for F– is 1.47×10-11 .

A: The reaction is as follows, The ICE table for above reaction is shown below,

Q: Nitrous acid is a weak acid and has a concentration of 0.65 mol/L. What is the pH of the solution…

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Q: The ionic strength of 0.30 M NaCl is: O 0.30 O 0.10 O 0.40 O 0.60 O 0.70

A: Given: Concentration of NaCl = 0.30 M Since NaCl is an ionic compound which will dissociate…

Q: Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic…

A: Henderson equation for acidic buffer solution: pH = pKa + log CH3COO-CH3COOH  (a) pH = 4.76 + log…

Q: Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion 1BrO-; Kb = 4.0 *…

A: Since the BrO- will get hydrolysed by water as per the reaction => BrO- (aq) + H2O (l)…

Q: What is the pH of a 6.65×102M aqueous solution of sodium hypochlorite, NACIO? (K, for HCIO =…

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: Calculate pH of a solution containing 0.50 M NaOCI and 0.75 M HOCI. (K, of HOCI = 3.2 x 10 8) O7.89…

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Q: For HClO2, Ka= 1.2 × 10-2. What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and…

A: Buffer solution is the solution which contains both acidic as well as basic part. The pH of buffer…

Q: The acid strength decreases in the series HBr > HSO, > CH3COOH > HCN > HCO, Which of the following…

A: The order of acidity of conjugate bases are same as the acidity of acids. But a strong acid has weak…

Q: Indicate whether each of these Lewis Acids is likely to form stronger bonds to fluoride or iodid and…

A: The given caions are Ag+, H+, Cu+, Ti4+, V5+. The above cations form strong bonds with either…

Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)

A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…

Q: A buffer solution is 0.318 M in HClO and 0.217 M in KClO . If Ka for HClO is 3.5×10-8 , what is the…

A: pH = pKa + log [salt]/[acid]

Q: Complete and balance the following acid–base and acid-carbonate reactions:(a) Al(OH)3+H2SO4

A: A chemical reaction is symbolic representation of the conversion of substances to new substances.In…

Q: What is the molar concenuration of hydronium [H,O*] ions in a solution prepared at 25°C with a pH of…

A: The acidic or basic nature of a solution is determined by its pH value. pH measures the…

Q: Calculate the pH of a 0.0325 M hypochlorous acid solution. [ K, = 3.0 x 10-8]. %3D O 9.49 O 4.51 O…

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Q: Calculate the pH of a 0.67 M solution of sodium nitrite (NANO,). K, (HNO2) =4.6 x 104 8.58 8.01 9.56…

A: pH of 0.67 M NaNO2 solution ( Ka of HNO2 = 4.6 X 10-4 )    First, write the equation for the…

Q: Supposed a 0.33 M aqueous solution of sulfuric acid (H2SO4) is prepared. Calculate the equilibrium…

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Q: The acid ionization constant for Fe(H 2O) 62+(aq) is 3 ×10-6. Calculate the pH of a 0.10 M solution…

A: Acid ionization constant denoted by Ka is the equilibrium constant measure of tendency of an acid to…