Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction.                                       HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH?   a. The flask will be pink b. The flask will be colorless c. The flask will be white from KCl precipitation d. There is insufficient information to solve this problem

Q: What change will be caused by addition of a small amount of Ba(OH) 2 to a solution containing CN-…

A: The solution is- H+(aq)+CN-(aq)↔HCN(aq) here Hydrogen ions are reacting with cyanide ions to form…

Q: A solution of sodium chlorite is prepared using 0.38 mol L1 NaOH as the solvent. The pK, of chlorous…

A: Solutions- Given- NaOH Conc. = 0.38 mol/lit, pKa of chlorous acid = 2, conc. of sodium chlorite =…

Q: Bromothymol blue is yellow in acid solutions. HBB is acidic form of the indicator. The indicator is…

A: Acid will react with base and base will react with acid and carryout neutralization reaction.

Q: Equal quantities of 0.010 M solutions of an acid HA and a base B are mixed. The pH of the resulting…

A: The chemical equation for the reaction between HA and B can be written as follows,

Q: A solution of phenol (HC6H50) is prepared by dissolving 0.385 g of phenol in 2.00 L of H2O. The…

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Q: Which of the following aqueous solutions are good buffer systems? 0.37 M potassium chloride + 0.24 M…

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Q: The table indicates how pH indicators change color based on the pH of the solutions that you put…

A: Given : pH range in which colour changes for bromothymol blue is 6.0 - 7.6. The colour change of…

Q: An analytical chemist is titrating 52.7 mL of a 0.3500M solution of methylamine (CH, NH,) with a…

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Q: Which of the following aqueous solutions are good buffer systems? 0.25 M ammonium nitrate + 0.37 M…

A: Acidic buffer: An acidic buffer is formed by the combination of a weak acid and its conjugate base.…

Q: An aqueous solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium…

A: Given: Buffer solution of hydrazoic acid i.e. HN3 and sodium azide i.e. NaN3.

Q: A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide (this…

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Q: Write the K expression for an aqueous solution of hypochlorous acid:

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Q: A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH…

A: This is actually a buffer mixture of weak acid (lactic acid) and it's salt(sodium lactate).…

Q: Which of the following will raise the pH of a strong acid HA in aqueous solution? I addition of…

A: I) Since HA is a strong acid  hence it will dissociate completely into H+ and A- ions And since pH =…

Q: An analytical chemist is titrating 107.8 ml. of a 0.1900M solution of dimethylamine ((CH,) NH) with…

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Q: Which salts will be more soluble in an acidic solution than in pure water? PbSO4, Ni(OH)2, CaCO3,…

A: Salts will be more soluble in acidic conditions when anion of the salt reacts with H+ of acid and it…

Q: The equilibrium concentration of zinc ion in a saturated zinc sulfide solution is ____ M.

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Q: One of the factors that can affect the pH of a buffered solution is the molar ratio of the conjugate…

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Q: Which of the following aqueous solutions are good buffer systems? 0.15 M calcium hydroxide + 0.26 M…

A: The following aqueous solutions are good buffer systems will be:

Q: The organic compound trishydroxymethylaminomethane is abbreviated Tris and is basic. The conjugate…

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Q: In the following chemical reaction what is the pH in a solution that is 0.00045 M [Al(H2O)6]3+.…

A: pH of the solution refers to the power of the hydrogen ion (H+) present in the solution.  It…

Q: Which of the following aqueous solutions are good buffer systems? O 0.22 M hydroiodic acid + 0.23 M…

A: Buffer solution is solution in which weak acid or weak base present with their conjugate acid or…

Q: Which of the following aqueous solutions are good buffer systems? O 0.17 M acetic acid + 0.21 M…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: A diprotic acid, H2A, has the following ionization constants: K = 1.1 x 10 and K =2.5 x 106. In…

A: Given: Ka1 of H2A = 1.1 × 10-3  Ka2 of H2A = 2.5 × 10-6  And pH of buffer required = 5.80

Q: Which of the following acids is the best choice to prepare a buffer at pH 9.4 when paired with their…

A: The value of pH for titration of weak acid with strong base is calculated by Henderson-Hasselbalch…

Q: The capacity of a buffer towards bases depends upon ... Multiple Choice the strength of the acid…

A: Solution :             Buffer capacity is defined as the efficiency of buffer to resist the change…

Q: Why does an indicator change from its acid color to its base color over a range of pH values? In…

A: indicators are the substance whoose solution changes colour due to Changes in PH. These are called…

Q: solutions.  BB- is  basic form of the indicator.             HBB    +     H2O          H3O+      +…

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Q: A buffered solution contains 0.50 M acetic acid (HC₂ H₂O₂. Ka 1.8 x 105) and 0.50 M sodium acetate…

A: We have to predict the new pH value after adding the base to buffer solution.

Q: This question is concerned with acid/base. The ionic product of water may be taken as 10-14…

A: Introduction: The Titration is provided a graph that is called titration curve which contains the…

Q: For each of the following salts, choose whether the resulting aqueous solution would be acidic,…

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Q: An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M…

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Q: An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M…

A: Titration of 111.3 mL of a 0.2800M solution of ammonia NH3 with a 0.3500M solution of HIO3 is…

Q: What is the pH (aq., 25 oC) above which a solution of iron(III) hydroxide will precipitate? Ksp =…

A: Given that,  Ksp of Fe(OH)3  = 2.60 x 10–39 A general dissociation reaction of Fe(OH)3 in water take…

Q: B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an…

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Q: The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to…

A: Since we know that if we dilute an strong acid solution it's pH will increase but if we dilute an…

Q: The equilibrium concentration of lead ion in a saturated lead iodide solution is M.

A: We know that Ksp is an equilibrium constant related to slightly soluble ionic compounds.   The…

Q: 6. Which of the following processes will increase the pH of a buffer solution prepared by mixing…

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Q: Thymol blue is a unique indicator that has two set of color change, red to yellow near pH = 1.5 and…

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Q: Which of the following aqueous solutions are good buffer systems?   A) 0.22 M hydrobromic acid +…

A: Buffer solution always resist the change in pH of solution. Buffer solutions are those that are…

Q: Which of the following aqueous solutions are good buffer systems? 0.19 M sodium hydroxide + 0.21 M…

A: The following aqueous solutions are good buffer systems will be:

Q: Calculate the equilibrium molar concentrations of trichloroacetic acid in an aqueous solution that…

A: Concentration in terms of molarity is defined as the moles of solute present per litre of the…

Q: For the buffer solution of weak acid HA and its conjugate base salt NaA, [HA] and [A] are expressed…

A: We are given a buffer solution of a weak acid and a conjugate base,

Q: Suppose you want to prepare a solution with a pH of 4.00 using acetic acid, CH3COOH, and sodium…

A: Given:  Ka  for acetic acid = 1.8 × 10-5  pH = 4.00

Q: Tin(II) oxide is amphoteric. Write balanced chemical equations for its reactions with an aqueous…

A: The "balanced chemical equation" for the reaction between tin(II) oxide and hydrochloric acid is…

Q: A chemist wishes to prepare a standard aqueous solution that has a concentration of Fe3+ equal to…

A: Please have a look into the solution:

Q: Lactic acid has a K. of 2.502 x 103. A solution contains 0.275 M lactic acid and 0.375 M sodium…

A: Buffer solution: The mixture of lactic acid and sodium lactate act as a buffer solution. The…

Q: Which of the following aqueous solutions are good buffer systems? O 0.29 M nitric acid + 0.24 M…

A: A good buffer consist of: weak acid + conjugate base salt Weak base + conjugate acid salt

Q: Acid Base Equilibria (Common Ion Effect) Determine the pH of (a) a 0.20 M NH3 solution, (b) a…

A: pH is defined as negative logarithm of hydrogen ion concentration. pH = − log [H+] A solution formed…

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.