A solution containing 2.00 mol Ca(OH)2 is titration with HCl. How many miles of HCl are required to teach the equivalent point.

Q: 7. You are given a 500 ml solution of 0.1 M HNO3 and an indicator HIn (Ka = 3.2x10) which changes…

A: The weak acids or bases that have different color in their dissociated and undissociated forms are…

Q: calculate the pH of the solution created by mixing 2 liters, 2 N, Ca (OH) 2 with 2 liters of 1 M…

A: Whenever anl strong acid and strong base reacts with each other than they neutralises each other to…

Q: A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide.  What is…

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Q: What is an acid–base indicator? Define the equivalence (stoichiometric) point and the end point of a…

A: An acid-base indicator is either a weak acid or weak base that exhibits a colour change as the…

Q: 75.0 ml of 0.0200M Ca(OH)2 solution is combined with 100.0 ml of 0.0150M NaOH solution.  Calculate…

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Q: Calculate the pH at the equivalence point for titrating0.200 M solutions of each of the following…

A: (a) Given, The concentration of NaOH solution is 0.200 M The concentration of HBr solution is 0.200…

Q: Determine the Concentration of Acetic Acid in Vinegar a this lah, you wil detarmine the…

A: Vinegar contains acetic acid. By titrating this with a base we can easily calculate the…

Q: How does the change of color in indicators define the acidity or basicity of solution put into it?

A: It is Substance in which acid or base is added then due to difference in pH indicators changes it's…

Q: The K, of hydroxylamine, NH,OH, is 1.10 x 108. A buffer solution is prepared by mixing 100.0 mL of a…

A: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its…

Q: In which case medium in Equivalent point is expected to be neutral: titration of H2SO4 by KOH…

A: The titration of strong acid with strong base gives a neutral solution at equivalence point. The…

Q: The useful pH range for a typical indicator is ________ 14 2 4…

A: pH is also called as the power of H+ ions. The pH value tells us about the acidic or the basic…

Q: Using a relevant ICE Table, calculate the expected pH of the solution when 5.99 mL of 0.200 M HCl…

A: Calculate the expected pH of the solution when 5.99 mL of 0.200 M HCl solution is added to the 50.0…

Q: A 0.338 g sample of an unknown triprotic acid dissolved in water is titrated to the second…

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Q: 2.1 The correct indicator was added to 25.00 mL of a 0.1340 M solution of pentanoic acid…

A: Pentanoic acid is a weak organic acid. Its Ka is 1.4 x 10-5.  Its concentration is 0.1340 M and…

Q: Determine the pH when 0.05mole of CO2 is dissolved into 1L of water. When 0.03 mole of sodium…

A: The carbon dioxide is a gas that dissolves n water upto a certain extent. There exists an…

Q: A 22.00 mL sample of HCl is titrated to phenolphthalein end point with 24.63 mL of a 0.08481 M NaOH…

A: Given :-  Molar concentration of NaOH = 0.08481 M  Volume of NaOH used = 24.63 mL  Volume of HCl…

Q: . Commonly used standards for the direct determination of the normality of an acid. 2. It is used…

A: Given:  1. Commonly used standards for the direct determination of the normality of an acid. 2. It…

Q: How many mL of a 5.0-M solution of sodium borate must be added to a 200-mL solution of 50 mM boric…

A: Pka of boric acid = 9.14    Cl+ consider x ml  5.0 M sodium borate is  required.   PH  = Pka +…

Q: to the solution containing 8 grams of Ca (OH) 2 in 50 ml of it add 500 ml of solution 0.1 mol HCl…

A: Given,  Mass of Ca(OH)2 = 8 grams Volume of Ca(OH)2 = 50 ml = 0.05 L Volume of HCl = 500 ml = 0.5 L…

Q: 25.00ml of 0.5M hydrobromic acid solution is titrated with 0.455M potassium hydroxide solution. what…

A: A neutralization reaction can be described as a chemical reaction in which acid and base reacts…

Q: What is buffer solution?give the application of buffer with proper solution.

A: To find: The definition for buffer solution Application of buffer

Q: A solution of nitric acid, HNO2, at a concentration of 0.495M was found to be 1.83 = pH.

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Q: A 40.0 mL sample of a 0.08 M HCl solution is titrated with a 0.10 M NaOH. What volume of tiltrant is…

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Q: Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq). What is the pH at…

A: The pH at the equivalence point has to be identified.

Q: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

A: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

Q: Which indicator could be used to titrate aqueous NH3 with HCl solution?

A: The difference between the endpoint and the equivalence point is the titration error, which should…

Q: Which graph best represents the titration of ammonia with hydrochloric acid?

A: Ammonia is a weak base and HCl is a strong acid . Titration of Ammonia with HCl is explained with…

Q: Which of these indicators is best suited to distinguish between a solution that is slightly acidic…

A: How to differentiate between slightly acidic and slightly basic solution with the help indicator?

Q: What is the pH at the equivalence point in the titration of 0.50 M KOH with 1.00 L of 0.750 M HF(aq)…

A: 1- First calculate the volume of KOH :  We will used the equation, ( M2V2)KOH = ( M1V1)HF  ( 0.50M ×…

Q: In titrating 40.0 ml of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: Given: Concentration of HCl = 0.10 M Volume of HCl solution used = 40.0 mL = 0.040 L…

Q: Calculate the pH at the stoichiometric point when 25 mL of 0.10 M pyridine is titrated with 0.32 M…

A: Moles can be calculated by using following formula,Moles = Molarity × Volume

Q: A student has a sea water sample which contains Ca2 ions . Describe briefly how he will determine…

A: To determine the concentration of calcium ions, we have to perform titration with EDTA solution. In…

Q: The beaker  contains 0.1 M acetic acid solution with methyl orange as an indicator. Another beaker…

A: A buffer is formed when a weak acid is mixed with its conjugate base or weak base with its conjugate…

Q: Describe the pH changes that occur during the titration of a weak base by a strong acid. What is…

A: A reaction between a base and an acid to give water and salt as products is known as the…

Q: b) 0.25 Lof an aqueous solution contains 0.35g Ba(OH), (171.34 g/mol). Calculate the Tonic strength…

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Q: A solution of K2CO3 was titrated with HNO3, Data was collected and a titration plot was constructed.…

A: …

Q: Derive the Henderson–Hasselbalch equation as a group. Take turns having each group member write and…

A: Henderson- Hasselbalch equation is used to determine the relation between the acid dissociation…

Q: Why is the pH at the equivalence point slightly different from that of the end point? Explain.

A: To explain: pH at the equivalence point is slightly different from that of the endpoint.

Q: In titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: Answer :- pH = 2.44…

Q: What is the effect of the ratio of conjugate base to acid on buffering capacity?

A: In essence buffer solutions resist changes in pH. A buffer contains appreciable amounts of a weak…

Q: Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 MBa(OH)2 with…

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Q: How does a buffer solution prevent larger change in pH? What does it mean when a solution has…

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Q: Explain the Buffer Range and Buffer Capacity?

A: Buffer range : pH range in which buffer solution can resist the change in pH effectively is known as…

Q: What factor governs the selection of an indicator for a neutralization titration? A) the final…

A: Indicator are used in acid base titration or neutralization titration to detect the end point of…

Q: 1.0.20 mol of KOH is added to 1.00 L of a solution that contains 0.50 M HC3H5O2 (Ka = 1.3 x 10) and…

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Q: A solution was prepared by mixing 50.0 mL of 0.10 M HCl and 25.0 mL of 0.25 M NaOH. What is the pH…

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Q: Define the term Buffer-Capacity?

A: The amount of acid or base required to raise the pH of a buffer by unity is known as its buffer…

Q: Suppose a titration was performed in which a base of pH 6 was being titrated. The equivalence point…

A: SOLUTION: Step 1: An indicator is chosen that has a pKa close to the pH at which the titration…

Q: Calculate the concentration of the acid, if 13.45 mL of 1M NaOH solution was needed to react with…

A: Given information, Volume (V1) of NaOH = 13.45 mL Concentration (M1) of NaOH = 1 M Volume of acid…