A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate (g) pK for the solution. (h) pFe(CN)6 for the soluti

Q: 4. (a) A laboratory technician dissolved 6.797 g of compound W (a non-electrolyte) in 15.00 mL of…

A: Please find the attachment.

Q: A student in conducting molecular weight determination of an uninown diprotic acid. He first…

A: KHP dissociates completely to form K+ and HP-. HP- then acts as weak acid. KHP and NaOH are…

Q: What is the pH of a buffer that is 0.200 M H2PO4−and 0.250 M HPO42− at 25°C?

A: The buffer solution is the solution that resists changing the pH of the solution if a small amount…

Q: Describe the solubility of CaF2 in each solution compared to its solubility in water.a. in a 0.10 M…

A: a). The ionization of CaF2 can be represented as: 0.10 M NaCl solution NaCl does not affect the…

Q: What is the mass solubility(g/100 mL) of Ca(OH)2 if a saturated solution has a pH of 11.95 at 25°C?

A:

Q: A solution is made by mixing 140.0 mL of 0.250 M BaCl2 and 120.0 mL of 0.400 M NaCl. What is the…

A: Given :- 140.0 mL of 0.250 M BaCl2 & 120.0 mL of 0.400 M NaCl solutions are mixed to give a…

Q: What are the [H₃O⁺] and the pH of a buffer that consists of 0.20 M HF and 0.25 M KF (Kₐ of HF…

A: pH is also known as potential of hydronium ion which we determine usually for a solution of…

Q: How many microliters of 1.000 M NaOH solution mustbe added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: In a gaseous equilibrium, the reverse reaction occurs whenQc> Kc. What occurs in aqueous solution…

A: The equilibrium constant (Kc) is the ratio of the product of the concentrations of the products to…

Q: A bioengineer preparing cells for cloning bathes a small piece of rat epithelial tissue in a TRIS…

A:

Q: How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: A buffer solution is prepared by dissolving 0.200 mol of NaH2PO4 and 0.100 mol of NaOH in enough…

A: pH is used to determine the concentration of hydronium ion.

Q: Suppose you wanted to make a buffer of exactly pHpH 7.00 using KH2PO4KH2PO4 and Na2HPO4Na2HPO4. If…

A: Henderson – Hasselbalch equation can be used here, i.e pH=pKₐ+log₁₀([A⁻]/[HA])

Q: 1. Calculate the volume, in mL, of a 0.50 M NAOH solution that will be required to titrate 1.2 of…

A:

Q: If 30 mL of 0.50 M OH- is added to 200 mLs of a 1.5 M buffer (pH 7.4), what is the resulting pH in…

A:

Q: What is the pH of a buffer made from 0.130 mol of HCNO (Ka=3.5*10^-4) and 0.410 mol of NaCNO in 2.0…

A: pH of the solution  = 3.96

Q: 2) How many grams of NaOH should be mixed with 5.4 g of oxalic acid (H,C.O.) and completed to 100 ml…

A:

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10-9) and 0.150 mol of KBrO in…

A:

Q: 100.0 mL of a 0.50 M aqueous NH3 solution is mixed with 200.0 mL of 0.25 M aqueous HCI. At 25 °C the…

A: Given : Concentration of NH3 = 0.50 M Volume of NH3 solution = 100.0 mL = 0.100 L…

Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ka = 2.5 × 10-9) and 0.130 mol of KBrO in…

A:

Q: Consider the titration of 17.50 mL of 0.459 M potassium propanoate, CH3CH2CO2K, with 0.107 M HNO3.…

A: Millimoles of propanoic acid form =0.107*39.38=4 .21 Millimoles of salt remain=17.50*0.459 -4.21…

Q: What is the pH of a buffer made from 0.140 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A:

Q: What will be the pH of a buffer prepared from 5.3 g of NH4Cl and 35 mLs of 1 M NaOH, diluted to a…

A: Buffer is a solution that resists the change in pH when small amount of acid or base is added to it.…

Q: A solution is 0.0111 M in both Br– and SO42–. A 0.270 M solution of lead(II) nitrate is slowly added…

A:

Q: An analyst was titrating a solution of unknown acetic acid concentration with 0.01 M NaOH using…

A: pH range of phenolphthalein indicator is 8.3 to 10 i.e below pH 8.3 it is colourless and above pH 10…

Q: What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (K, = 1.8 x 10$)?

A: Given : Concentration of weak acid CH3COOH = 0.15 M And concentration of conjugate base salt of weak…

Q: 16.5 mL of 0.1000M HCI are required to titrate a 10.00 mL aliquot of a saturated strontium hydroxide…

A: The productof the ionic concetrations of a electrolyte that at one temperature can continue in…

Q: From the value of Kf, calculate the concentration of NH3 required to just dissolve 0.020 mol of…

A:

Q: What is the component concentration ratio, [CH₃COO⁻]/[CH₃COOH], of a buffer that has a pH of 4.39…

A: The dissociation of weak acid takes place as follows: HA+H2Ol⇌H3O++A- The expression for the…

Q: (3) How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid…

A: Molarity of buffer to be prepared [AH] = 0.750 M Volume of buffer solution = 500 ml pH of buffer…

Q: A 4.0520g sample of hydrochloric acid, sp.gr 1.18, required 44.15ml of 0.9035N sodium hydroxide in a…

A:

Q: What is the pH of a buffer that is 0.12 M HNO2 and 0.16 M NANO2 and the pKa is 3.35?

A:

Q: What is the pH of a buffer that is 0.15 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A:

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Using details from the question, the number of moles of HNO3(nitric acid) titrated, can be…

Q: What is the pH of a buffer made from 0.200 mol of HCNO (Ka = 3.5 × 10-4) and 0.410 mol of NaCNO in…

A: Given, the number of moles of HCNO =0.200 molenumber of moles of NaCNO =0.410 molevolume of solution…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Given : concentration of HNO3 used = 0.340 M Volume of HNO3 solution used = 19.6 mL

Q: Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.…

A: Given: [NH3]=0.50 M[NH4Cl]=0.20 MpKb=4.75Volume of solution=1.0 L To calculate: pH

Q: A 5.00 mL sample of drinking water contains 15% by weight CI, was titrated with 0.1M AgNO3 using…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2,M(OH)2, is mixed with pure water.…

A: Given that,PH of the solution = 10.28Ksp =?You know thatPH + POH = 14

Q: What is the pH of the buffer that results when 3,06 g of NagHPO, and 2.17 g of NaH,PO, are diluted…

A: Mass of Na2HPO4 = 3.06 g Mass of NaH2PO4 = 2.17 g Volume of buffer solution = 0.3 L Ka of H2PO4- =…

Q: A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K = 4.57x10) is titrated with 1.20 M NaOH…

A: 1.) First we would calculate moles and draw ICE table for reaction between acid and base.  Then we…

Q: The pKa of hypochlorous acid is 7.530. A 59.0 mL solution of 0.133 M sodium hypochlorite (NaOCl) is…

A: 59.0 mL of 0.133 M sodium hypochlorite (NaOCl) is titrated with 0.323 M HCl solution. The pKa of…

Q: Consider the following buffer system: 0.96 M H2CO3 and 1.08 M HCO3-. What is the pH of such a system…

A:

Q: 12. How much H;PO4 and NaOH are needed to prepare a buffer containing 0.40 mole HPO2- and 0.50 mol…

A: Given: Moles of HPO42- required in buffer = 0.40 mol. And moles of PO43- required in buffer = 0.50…

Q: What is the pH of a buffer solution prepared by dissolving 33.7 g NaCH3COO in a sufficient volume of…

A: Solution -

Q: How many grams of NH4CI would have to be added to 250.0 mL of a 0.420 M NH3 solution to prepare a…

A: The minimum concentration of NH4Cl that must be present in the solution to have a pH of 10 is;…

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.