Calculate the equilibrium concentration of Ni²* in a solution with an analytical NİY2- concentration of 0.0100 M at pH 2.0 and pH 9.0. K; of NIY2= 4.2 x 1018

Q: The digestion of a 0.1387-g sample of a phosphorus containing compound in a mixture of HNO, and…

A: Solution: Given: Mass of the sample containing phosphorus = 0.1387 gMolarity of NaOH solution =…

Q: How the aqueous chemistry of amphoteric hydroxides involves precipitation, complex-ion formation,…

A: The aqueous solution is the one in which the solvent is water. Different chemical reactions can be…

Q: If 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium…

A: Given, The mass of the AgBr = 316.0 mg The concentration of ammonia (NH3) = 0.12 M The volume of the…

Q: Calculate the Kc of the reaction below if the equilibrium concentrations of Ag and IO; are both 1.78…

A:

Q: 6. Given the following equilibrium reaction of NH3: NH4+ (aq) + OH (aq) NH3aq) + H₂O (1) Determine…

A: Given, NH3(aq) + H2O(l) <---> NH4+(aq) + OH-(aq) Concentration of NH3 solution (C) = 1.25 M Ka…

Q: In the determination of iron in limonite, 0.5166 g of mineral is dissolved in acid and Fe2 + is…

A: Amount of limonite = 0.5166 g 42 96 ml of 0.0213 M Na2Cr2O4 is added in the titration. Molar mass of…

Q: Group III (Al3+, Cr3+, Fe3+, Zn2+) cations produce very soluble sulphides so they can be…

A: The Group III cations include Al3+, Cr3+, Fe3+, Zn2+, Ni2+, Co2+ and Mn2+ ions. The solubility of…

Q: During the course of the titration of a 20.0 ml of solution containing 0.1 M of NaOH and 0.08 M of…

A: Initial moles of strong base, NaOH in the solution = C*V = 0.1 molL*20.0 mL = 2.0 mmol Initial moles…

Q: Total Acidity (mol/L) = [H+] + 2×[H2CO3-] + [HCO3-] - [OH-] Calculate the molar concentration of…

A:

Q: 8. Balance the following equations: (a) SO₂ + 0₂ - SO3 (b) Li₂O(s) + H₂O(1) LiOH(aq) (c) Na + H₂O…

A: Note: As per bartleby guidelines, solutions of first 3 questions has been made. For the exper…

Q: Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine,…

A: According to the question, The molarity of the triethylamine is given by = 0.1 MThe volume of the…

Q: What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid…

A: We have to predict the pH of buffer solution.

Q: A mixture containing 0.10 M KBr(aq) and 0.22 M NaF(aq) is electrolyzed. What is formed and why?

A: During electrolysis, oxidation takes place at anode and reduction takes place at cathode. Hence all…

Q: A sample of water has a pH of 5.3. The concentration of bicarbonate (HCO3-) in the sample is 190…

A: The concentration of hydrogen ion and hydroxide ion in mg/L is; H+=10-5.3H+=10-5.3 mol/L×1g/mol×1000…

Q: Calculate the pH of a 0.021 M CN - (aq) solution. [Ka(HCN) = 4.9 × 10-10]

A: Answer :

Q: Create the flowchart of qualititative analysis of Cations in Group 2 and explain.

A: Group II (Cu2+, Bi3+, Cd2+, Hg2+, As3+, Sb3+, Sn4+) cations produce very insoluble sulfides (Ksp…

Q: Quiz 1 Free Response Propose a synthesis of the target molecule below. You must show every…

A: Oxidation of primary alcohol gives aldehyde with mild oxidizing agent like PCC and PDC while with…

Q: Q3. 1.5g of 0.1M NaCl has been prepared in 1L and only 25 of NaCl solution has been used to titrate…

A: Introduction: Percentage yield if the ratio between the actual yield of chemical species to the…

Q: 3) In the treatment of myasthenia gravis, 10 mg of guanidine (NH-C(NH2)2) per kilogram of body…

A:

Q: The formation constant for FeY2−  is 1014.30. Calculate the concentration of free Fe2+ in a 0.560 M…

A: Given Concentration of FeY2- = 0.560 M

Q: calculate the ph and poh of a solution that is 0.18 M in HC2H3O2 and .43 M in Mg(C2A3O2)2 where the…

A: pH of a solution is defined as the negative logarithm of concentration of H3O+ ion. Again pH + pOH =…

Q: A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard…

A: Given: Volume of sample = 10.00 mL = 0.010 L                                (Since 1 L = 1000 mL)…

Q: When 15.11 ml of 0.102 M K2SO4 solution reacts with 35.00 ml of 0.114 M Pb(C2H3O2)2. predict the…

A: Data given: Volume of K2SO4 solution = 15.11 mL = 0.01511 L (1 L = 1000 mL) Concentration of K2SO4…

Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…

A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…

Q: What is the pH of a 0.820 M solution of Ca(NO2)2 (Ka of HNO₂ is 4.5 × 10-4)?

A:

Q: Calculate the pH of a blood plasma sample with a total CO₂ concentration of 24.0 mM and bicarbonate…

A: Concentration of CO2 = 24.0 mMConcentration of bicarbonate = 23.0 mmpKaCO3 = 6.10

Q: In finding the pH of the solution containing amphiprotic salts, diluted solutions contain…

A: Concentration of NaHCO3 solution = 0.1 (M)Ka1 = 1.5*10-4, Ka2 = 4.69*10-11

Q: 5. The dichromate ion, Cr2O72- reacts with methanol, CH3OH in acidic solution according to the…

A: Final volume = 200 x 3 = 600 mL [Cr2O72-] = 200 x 1 / 600 = 0.33 M [CH3OH] = 200 x 1.875 / 600 =…

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: 2. There is a phosphate buffer with 0.1 M of NaH2PO4 0.1 M of Na2HPO4. Calculate pH of buffer…

A: pH of a buffer solution can be calculated using H-H equation.

Q: A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?

A: Given pH = 3.7 Initial Concentration = 0.020 M

Q: (8) Answer each of the following questions: (a) Ka for HNO₂ is 4.6 x 10-4. What is the Kb for its…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH of a…

Q: What is the pH of a 4.80x10-2 M aqueous solution of ammonium bromide, NH4Br? This solution is C pH =

A:

Q: Explain why K2CrO4 is used as an indicator in Argentometric titration

A: Argentometric titration is the titration method, which is used for the detection of halides or…

Q: Determine the pH at the equivalence point of a titration of 100.0 mL of 0.265 M CH₂NH₂ solution with…

A: Answer: Conjugate acid of weak base gets hydrolyzed in water and produces H3O+ ion and as CH3NH2 is…

Q: (Fe): 56 g /

A: Molarity of Na2Cr2O7 = 0.0213 M Volume of Na2Cr2O7 = 42.96 mL At equivalent point,  Geq. of Fe2+  =…

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: Determine the pH of a 0.0525M Fe(NO3)3 solution.  Ka of Fe3+ = 6.3x10-3

A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.

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: What is the Ph of the buffer solution that contains 1.00 M HC2H302 (acid) and 0.800 M KC2H302 with…

A: Whenever the acid concentration as well as its conjugate base, or the base and its conjugate acid,…

Q: What is the pH of a river water sample in which [HCO3-] = 1.0 x 10-4 M and the concentration of…

A: The given river water sample in which [HCO3-] = 1.0 * 10-4 (M) and the concentration of dissolved…

Q: Complete the balanced dissociation equation for the compound below in aqueous solution. Rb 3PO4 (S)…

A: A balanced equation is one in which the number of atoms on both side of the equation are same. A…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.