To adjust the EDTA solution, a 0.01 M 10 mL Ca+2 sample was taken and 10 mL of pH 10 buffer was added to it, and the volume was completed to 100 mL. Then, two drops of EBT indicator were added and titrated with EDTA. Since the consumption is 10.4 mL, which of the following is the concentration of the EDTA solution in terms of molarity?

Q: What would be the pH values when (a) 0.0090 mol HCl and (b) 0.0090 mol NaOH, added to 0.300 L of a…

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

Q: A 1.000 L solution buffered at pH = 4.3000 was prepared by mixing certain volumes of 0.5000 M HNO2…

A:

Q: Find the pH of the equivalence point(s) and the volume (mL) of 0.447 M HNO3 needed to reach the…

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

Q: 0.3 g of a weak acid was dissolved in 75 mL water. Phenolphthalein indicator was added. 0.1 M…

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Q: An unknown solution is red with phenol red and colourless with thymolphthalein. From that…

A:

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: We titrated crotonic acid (weak acid) with HCl, using a conductivity titration (Part 1) to the…

A: Crotonic acid is a weak acid and a short chain unsaturated carboxylic acid . HCl is hydrochloric…

Q: Determine the volume in mL of 0.652 M CSOH(aq) needed to reach the half-equivalence (stoichiometric)…

A: Given : Concentration of CsOH = 0.652 M Concentration of HBrO = 0.873 M And volume of HBrO solution…

Q: emistry A 110.0-mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. The Kb value for NH3 is…

A: The answer is as follows:

Q: in an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this…

A: Given that : The mass of Ca = 0.050 g The volume of DI water = 150 mL The molarity of HCl = 0.30 M

Q: Which of the following systems would make an effective buffer? 50.0 mL of 1.0 M NaHSO3 with 60.0 mL…

A: Effective buffer is effective when the amounts of acid/ base should be more than there conjugates.

Q: Which is the best colored indicator to use in the titration of 0.1 M NH3(aq) with 0.1 M HCl (aq)?…

A: Which one of the correct

Q: bottle of acid in the lab is found. It is labelled as oxalic acid (H2C2O4). There is no…

A: In this question, we will see that which methods we can used to determine the Concentration of…

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: 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: Suppose a back titration occurs that consists of 1.895grams of CaCO3 antacid (assume no buffer). The…

A: Introduction: As per the international system of unit (SI), mole is the unit of measurement for the…

Q: Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant…

A: The reaction of Na2CO3 with HCl is, Na2CO3 + 2HCl = 2NaCl + CO2 + H2O Given Formula mass of Na2CO3 =…

Q: Use acid-base titration to determine the concentration of: – A strong acid: HCl 0.100 M NaOH…

A: Given : Concentration of NaOH used = 0.100 M Volume of NaOH solution required to reach endpoint i.e…

Q: Give typed full explanation not a single word hand written otherwise leave it  An experiment…

A: Sodium acetate (NaC2H3O2) is a salt of weak acid acetic acid(HC2H3O2). When in a solution weak acid…

Q: Acid Base Tritation When 25.00 mL of HNO3 are titrated with Sr(OH)2, 58.4 mL of a 0.218 M solution…

A: A) before titration first Calculate mole of Sr(OH)2 then use Mole-mole realtionship to get mole of…

Q: A purified protein is in a 100. mM HEPES buffer pH 7.3 with 500. mM sodium chloride (NaCl). A 25.0…

A: Given that: pH = 7.3 Concentration of HEPES with NaCl = 100 mM  Concentration of NaCl in HEPES…

Q: (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the…

A: Answer: Given curve is the titration curve of acid and base titration where acid is the analyte and…

Q: Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb =…

A:

Q: The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid…

A: Step :

Q: Predict whether the equivalence point of each of the followingtitrations is below, above, or at pH…

A: The point at which the amount of titrant added is sufficient enough to neutralize the analyte…

Q: 10.00mL of O.10M HCI were collected in an Erlenmeyer flask, and 100mL with distilled water. After…

A: HCl is an acid and NaOH is a base and both react to form salt and water. The H+ ions dissociated…

Q: Calculate the pH at the equivalence point in titrating 0.020 M solutions of each of the following…

A: pH is the power of hydronium ion concentration. It is used to measure the acidity or alkalinity of a…

Q: Draw the titration curve that would result if 35 mL of a 0.2 M CH3NH2 (kb = 4.60 x 10-4) were…

A: [CH3NH2] = 0.2 M Volume of CH3NH2 = 35 mL                            Kb = 4.60 *…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.50E-05 at 25°C) is titrated with…

A:

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

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

Q: Reaction HA(aq) + H20(1) H;O°(aq) + A (aq) Initial conc. / M: 0.0900 Change in conc. at equilibrium…

A: pH  - It is known as the negative logarithm of the hydronium ion concentration of a solution. Ka -…

Q: Calculate the pH at the equivalence point in titrating 0.021 M solutions of each of the following…

A:

Q: What is the best way to calculate the following titration: 100 ml water and 100 ml of solution…

A:

Q: biochemist is trying to prepare 800.0mL of buffer using KH2PO4 and K2HPO4 combination, pKa for these…

A: To find the mass in grams of KH2PO4 and K2HPO4 that is required to prepare a buffer solution 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: Question No. 2: Calculate the pH changes during the titration of 0.0100 M NaOH with 50.00 mL of…

A: The balanced neutralization equation is: NaOH(aq) + ClCH2COOH(aq)  ----> ClCH2COONa(aq) + H2O(l)…

Q: A 1.000 L solution buffered at pH = 4.3000 was prepared by mixing certain volumes of 0.5000 M HNO2…

A:

Q: A 116.2 mL sample of 0.120 M methylamine ( CH3NH2; Kb = 3.7 x 10-4) is titrated with 0.240 M HNO3.…

A:

Q: The protonated form of the indicator (Hln) is red. Hln dissociates into a yellow, deprotonated…

A: Answer: Indicator is a chemical substance that changes its color during the titration to indicate…

Q: A buffer solution is made that is 0.322 M in HCN and 0.322 M in NaCN. (1) If K₂ for HCN is…

A:

Q: 30 cm3 of 0.5 M solution of weak monoprotic acid titrated with 10 cm3 of a 1 M NaOH solution. If the…

A:

Q: analytical chemistry. Given the following titration curve, what is the suitable indicator for this…

A: The above question is based on analytical chemistry . We have to discuss about the roll about the…

Q: (2) A student titrates 25.00 ml of 0.200 M acetic acid (Ka = 1.8 x 10) with 0.200 M NaOH. Calculate…

A: Balanced equation for the reaction of NaOH and acetic acid(AcH) is: AcH(aq) + NaOH(aq)  ---->…

Q: A 50.0 ml aliquot of a 0.0010OM solution of acetic acid (K = 1.8 x 10-5) is titrated with 0.00993M…

A:

Q: Which of the following indicates buffering in the titration given in the image below? 12 11 10 Point…

A: The word buffer has the ability of being able to resist drastic changes in pH upon addition of…

Q: A 0.2014 g of the primary standard Na2CO3 (105.99 g/mol) required 37.00 mL of HCl (36.45 g/mol) to…

A: First write the balanced reaction for Na2CO3 and HCl. Then use mol to mol ratio to find moles of HCl…

Q: When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an…

A: The question is based on the titrations.  we are titrating a weak acid acetic acid with a strong…

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