A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 M Na2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown.

Q: aOH. Calculate the pH of the solution after the addition of 29.7 mL of NaOH s

A: A) mmoles of Acid ( HN3 ) = 50.0mL • 0.217molL-1 = 10.85 mmol  B) mmoles of NaOH ( Base ) = 29.7mL •…

Q: A 5.850-g sample containing KCl and KClO4 was dissolved in sufficient water to give 250.00 mL of…

A: Given , Reaction : 8V3+ (aq) + ClO4- (aq) + 12H2O (l)→Cl- (aq) + 8VO2+ (aq) + 8H3O+ (aq) Volume of…

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 0.240 M pyridine, C,H,N(aq)…

A: pH of acid base titration can be calculated using respective formulas based on the point of…

Q: mount of X used in titration: 100.0 mmol amount NaOH added (mmol) (b) 35.0 220.0 (c) pH 2.558 4.482…

A: We have following formula -  pH = pKa + log [A-]/[HA]    Then -  (a)  pH = pKa + log [A-]/[HA]…

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Moles of base taken =Molarity of base×Volume of base=0.0200 mol/L×50.00×10-3L=0.001 mol

Q: Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.…

A: Molar concentration is the measure of the concentration of a chemical species, in particular of a…

Q: A buffered solution was prepared by dissolving 6.85g of sodium formate (NaHCOO in 250.0mL (16) of a…

A:

Q: 10.71

A: Molarity of HCl(M)= 0.050 M Volume of HCl(V) = 25 mL Mmol of HCl =  M × V      = 0.050 × 25 = 1.25…

Q: Can you explain the problem?

A: Step 1: Step 2: Step 3: Step 4:

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Given: Weak base = 0.0200 M Volume of weak base = 50.0 mL Concentration of base = 0.0150 M pKb of…

Q: Calculate the molar solubility of iron(II) hydroxide in an aqueous solution buffered at pH = 6.07.

A:

Q: Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 MHNO2 by…

A: Given:Concentration of HNO2 = 0.100 MConcentration of KOH = 0.200 MVolume of HNO2 = 40.0 mLpKa of…

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

A: According to the Law of conservation of mass " all atoms of different elements must be equal on both…

Q: Buffer preparation: A 6.90 g sample of sodium nitrite (NaNO2, 68.995) was dissolved in about 100. mL…

A: Given,  When 6.90g of NaNO3 was dissolved in 100.0 mL of water then added to 500mL of 0.200 M HNO2…

Q: Nitesh

A: The objective of the question is to understand the effect of adding a strong acid (HCl) to a buffer…

Q: Calculate the pH of a buffer solution containing 0.25 M NH3 and 0.34 M NH4NO3. Data: pKa (NH4+) =…

A:

Q: NH4

A: Given: Ammonia buffer solution: M1 =  0.25 M [NH4+] M2   = 0.22 M [NH3] pKa of NH4+ = 9.24

Q: Determine the pH during the titration of 39.6 mL of 0.226 M trimethylamine ((CH3)3N, Kp = 6.3x10-5)…

A: Since you have asked a question with multiples of parts we will answer only 1st 3 subparts for you.…

Q: A 0.1504-g sample of impure Na₂CO₃ (106.00g/mol) was analyzed via Volhard method. After adding 50.0…

A: Here we are required to find the purity of Na2CO3.

Q: An ammonia buffer solution contains 0.20 M NH4+NH4+ and 0.21 M NH3NH3 . The pKa of ammonium is…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: Please provide detailed solution and give explanation of the concept

A: We are asked to find the volume of 1.35 M HCl that must be added to 0.264 L of 0.213 M dimethylamine…

Q: Calculate the volume of KOH required to reach the equivalence point-

A: Formula :-  MacidVacid = MbaseVbase   Acid = HNO3  Base = KOH

Q: Buffer preparation: A 6.90 g sample of sodium nitrite (NANO2, 68.995) was dissolved in about 100. mL…

A: Given,  When 6.90 g sample of NaNO2 was dissolved in 100.0 mL of water and it is added to 500. mL of…

Q: A 15.00 mL sample of 0.355 M H3PO4 (Ka,1 7.52 ´ 10–3 , Ka,2 6.23 ´ 10–8 , Ka,3 2.1 ´ 10–13) is…

A:

Q: A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2. Calculate the pH of the…

A:

Q: Consider the titration of 100.0 mL of 0.130 M H2NNH2 (Kb= 3.0 x 10-6) by 0.260 M HNO3. Calculate the…

A: First consider the volume of 0.0mL added. The ICE table for the reaction is as follows,

Q: Calculate the mas of KC2H3O2 that must be added to 500.0mL of a 0.200 M HC2H3O2 (Ka = 1.8 x 10-5)…

A: Given→ Volume of HC2H3O2  = 500.0 mL                Molarity of HC2H3O2 = 0.200 M                Ka…

Q: Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is…

A: Since you have posted a question with multiple sub-parts, we will provide the solution only to the…

Q: You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an…

A: The concentration and the number of moles of Ca2+ ion in the filtered solution is;…

Q: 3. (a) Is it possible to measure SO3 in the presence of OH (each with a concentration of 0.1 M) by…

A: Titration is an analytical method that is used in quantitative analysis to determine the amount of…

Q: A buffer was prepared by mixing 50.0mL of 0.10 M HX and 25.0mL of 0.10 M NaOH. The Ka of HX is…

A:

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for