100.0 mL sample of drinking water was buffered with ammonia at pH 10 and after addition of EBT required 21.4 mL of 0.00512 M EDTA for titration. FW CaCO3 = 100.09 g/mol. What will be the change in color at the end point? What is the water hardness in terms of ppm CaCO3

Q: . In a titration of a strong base with a weak acid at 25oC, the theoretical pH at equivalence point…

A: In a titration of a strong base with a weak acid at 25 oC, the theoretical pH at equivalence point…

Q: 50.0 mL of 0.0500 M HCN (K3=4.9x10-10) is being titrated with 0.0500 M Ba(OH)2 . Please answer the…

A: Given,  Molarity of HCN = 0.0500 M  Volume = 50.0 mL  Acid dissociation constant of HCN = Ka = 4.9 x…

Q: Explain the significance of Henderson-Hasselbalch equation in potentiometric titration of a weak…

A: The Henderson-Hasselbalch equation provides a relationship between the pH of acids (in aqueous…

Q: Calculate the needed reagents in preparing 250mL of 0.200M KH2PO4-K2HPO4 buffer with pH of 7.40.…

A: Given: Total concentration of soluion = 0.200 M Volume of solution = 250 mL = 0.250 L…

Q: Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 0.10 M H3PO4…

A: HCl neutralizes NaOH according to the equation: HCl + NaOH → NaCl + H2O The reaction between H3PO4…

Q: What volume of 1.35 MHCI must be added to 0.287 L of 0.323 Mdimethylamine to produce a buffer with a…

A:

Q: What is the molar solubility of NiS in 0.40 M NH3? The Ksp for NiS is 3.0 × 10-19. The K₁ for…

A: Two equations can be represented as; NiS  ⇌ Ni2+  +  S2-    ...KspNi2+ + 6NH3  ---->…

Q: A mixture contains initially benzoic acid C6H5CO2(weak acid), Ka = 6.28 x 10^-5, and its…

A: Given data :  Ka of benzoic acid = 6.28 x 10^-5 , concentration of benzoic acid = 0.250 M…

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: . Consider the titration of 15.0 mL of 0.150 M (C2H5)2NH(aq) (Kb= 6.9 x 10-4) with 0.125 M HCl(aq).…

A: Given:-          Volume of (C2H5)2NH=15.0 mL       Concenentration of C2H52NH=0.150 M…

Q: 1. A 100 mL volume of 0.10 M H₂A, a diprotic acid, is titrated with 1.0 M KOH. The diprotic acid has…

A:

Q: A 0. 238 g sample contained only NaCı and KBr. It was dissolved in water and required 48. 40 ml of…

A:

Q: A 40.00-ml aliquot of 0.2000 M HCI is titrated with 02000 M NaOH Calculate the pH of the solution…

A:

Q: Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4…

A: HCl vs NaOH Volume of HCl ( Va ) =25.00 mL Molarity of HCl ( Ma ) = 0.060 M  Molarity of NaOH ( Mb…

Q: For the titration of 50.00 mL of 0.300 M RbC7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x…

A:

Q: How much 6.01 MNaOH must be added to 520.0 mL of a buffer that is 0.0195 Macetic acid and 0.0240 M…

A: Given- Volume of buffer = 520.0 ml Concentration of acetic acid = 0.0195 M Concentration of sodium…

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

A: First, we need to calculate the pOH of the solution. The pH and pOH of a solution are related by the…

Q: A 20.0 mL sample of 0.115 M sulfurous acid (H2SO3) solution is titrated with 0.1014 M KOH. At what…

A: Given,A 20.0 mL sample of 0.115 M sulfurous acid (H2SO3) solution is titrated with 0.1014 M KOH.

Q: For the titration of 50.00 mL of 0.300 M RbC7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x…

A:

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

A:

Q: A 1.0 L buffer solution initially contains 0.25 mol NH3 (Kb=1.8x10^-5) and 0.25 mol of NH4Cl. In…

A: First we would Calculate Initial pH of buffer using Henderson Hasselbalch equation.  Then we check…

Q: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl.  Carbonic acid (H2CO3) has a…

A:

Q: A 13.0 ml solution of weak base with Kb = 1.33×10-3 (at 25°C) with concentration of 0.086 mol L1 was…

A:

Q: Calculate the silver ion concentration in terms of pAg during the titration of 70.00 mL of 0.07000 M…

A: The balanced chemical equation for the reaction between NaCl and AgNO3 is: NaCl + AgNO3 → AgCl +…

Q: What is the molar solubility of Tl2S in deionized water relative to the molar solubility of Tl2S in…

A:

Q: The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is

A: Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: 0.0500M

A: The objective of this question is to show the equivalence point is reached when the amount of AgNO3…

Q: pH Titration Curve for titrating 64.0 mL of Nitric Acid with 0.700 mol/L Aqueous Potassium Hydroxide…

A: From the pH vs volume of titrant we can figure out pH and Molarity of nitric acid.

Q: Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water.  Its Ksp is 2.8 x 10-20. In the…

A: Upon dilution, the number of moles in the solution remains constant whether the change in the…

Q: A student titrated 30.00 mL of a weak base solution, 0.150 M CH3NH2 (Kb = 4.40 x 10 4), with 0.100 M…

A:

Q: 2. Draw a graph of pH vs Vh for the titration of a strong acid with a strong base and compare it to…

A:

Q: Consider the titration of 20 mL of 0.105 M H3C2O2H(acetic acid) with 0.125 M KOH. Find the initial…

A: The objective of this question is to calculate the pH at different stages of a titration between…

Q: How many grams of NaC3H6O3 should be dissolved in 500.0 ml of 0.100 M HC3H6O3 (lactic acid) to make…

A: An acid buffer is a mixture of a weak acid and its salt with a strong base. It is given that pH of…

Q: What mass of NH4Cl (Mw = 53.492 g mol-1) has to be dissolved in 750 mL of 0.25 M NH3 (pKa = 9.26) to…

A: 750 mL of 0.25 M NH3 pKa = 9.26 solution is mixed with a certain amount of NH4Cl to prepare 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