In a titration experiment a 25.0 mL sample of a diprotic acid required 30.0 mL of 0.200 M NaOH for the endpoint to be reached, what is the concentration of the acid?

Q: In a titration experiment, 50mL of HCI was needed to completely neutralize 20mL of 0.25 M NaOH.…

A: Given :- Molarity of NaOH solution = 0.25 M Volume of NaOH solution = 20 mL Volume of HCl solution =…

Q: 50.0 mL sample of 0.10 m HCl is titrated to the end point buy 30.0 mL of NaOH. What is the…

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Q: A solution is prepared by mixing 585 mL of 0.600 M NH3 and 320 mL of 0.600 M HCI. Assuming that the…

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Q: 50 ml HCl solution requires 25.5 ml, 0.015 M Ca(OH)2 for the endpoint with a basic indicator. What…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: What is the resultant pH after mixing 30.0 mL of 0.50 M HCI with 20.0 mL of 0.90 M NaOH? Express…

A: Given: Concentration of HCl = 0.50 M Concentration of NaOH = 0.90 M Volume of NaOH solution = 20.0…

Q: to answer all parts A 10.0-mL solution of 0.870 M NH, is titrated with a 0.290 M HCI solution.…

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Q: What is the pHH a this buffer Suution?

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Q: A few mL of 0.800M HCl are added to 20mL of 0.800. NaC2H3O2. Will the initial pH of the 0.800M…

A: pH is used to determine the concentration of hydronium ion. pH for acid is less than 7. pH for base…

Q: To a 150.0 ml solution of 0.100 M NH3 solid NH4Cl is added. What will happen to the pH, [H+], [NH3],…

A: The aqueous solution of ammonia consists of ammonium ions. The dissociation constant of base can be…

Q: A 25.00-mL sample of an HNO3 solution is titrated with 0.102 M NaOH. The titration requires 28.52 mL…

A: The acid base reaction is HNO3 + NaOH -------> NaNO3 + H2O  Equivalent moles of acid and base…

Q: 30 ml of a 0.4375 M HCl solution are added to 35 ml of 0.250 NaOH solution. What is the final pH ?

A: given :-  molarity of HCl solution = 0.4375 M  volume of HCl solution = 30 mL  molarity of NaOH…

Q: A solution of oxalic acid is used to titrate 17.11 mL of a 0.5003 molar: sodium hydroxide. If the…

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Q: An aqueous solution of 0.1 M hydrochloric acid with a volume of 200 milliliters is mixed with 100 mL…

A: Moles of HCl taken = molarity of HCl X volume of HCl solution taken in L Since molarity of HCl = 0.1…

Q: A 150.00 mL volume of HCI solution required 29.71 mL of 0.01963 M NAOH to reach an end point with…

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Q: A mixture is made by combining 110 mL of 0.015 M HCl and 215 mL of 0.025 M HI. What is the pH…

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Q: Calculate the concentration of phosphoric acid in a solution if 25.0 ml of that solution required…

A: The balanced equation can be shown below

Q: How many ml of NaOH stock solution have been added to establish the buffer?

A: To prepare the desired buffer solution, at first, an acetic acid solution was taken and NaOH was…

Q: In the laboratory a student measures the percent ionization of a 0.532 M solution of benzoic acid,…

A: Given: Initial concentration of benzoic acid = 0.532 M percent ionization = 1.05 %

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: A solution is prepared by mixing 25 mL of 0.06 M NaOH with 65 mL of 0.125 KOH. What is the pH of…

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Q: A 0.605 gm sample of Sodium Carbonate and Sodium bicarbonate , the solution titrated with 0.106N HCI…

A: Solution: First write the balanced equations for titration of HCl with sodium carbonate and sodium…

Q: In titration of 50 ml of 0.1 M NaOH solution with 0.2 M HCl, which is the pH after adding 30 ml of…

A: For the given titration the volume of NaOH solution is 50 mL and the molarity of the NaOH solution…

Q: A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH. a) Calculate the pH at 25 mL…

A: given, volume of sample = 30.0mL                volume of base added = 25mL                molarity…

Q: A buffer solution of 200 mL is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX.…

A: Buffer solution :- A solution which resists change in its pH value by the addition small amount of…

Q: A 4.50−g quantity of a diprotic acid was dissolved in water and made up to exactly 250 mL. Calculate…

A: Given,Diprotic acid = 4.50 g in 250 mLKOH = 12.0 ml of 1.00 M.

Q: A 15.0 mL sample of HCI (acid) required 28.0 mL of 0.25 M NaOH (base) to reach the egyiyalence…

A: Given, volume of HCl (acid) (Va) = 15.0 mL. Volume of NaOH (base) (Vb) = 28.0 mL. Concentration of…

Q: What is the pH at the equivalence point

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Q: Suppose you are performing acid-base titration with HCl and NH4OH, select your indicator with…

A: In case of Strong acid and weak base just like HCl and NH4OH we use indicator methyl orange since it…

Q: If a buffer solution is 0.280 M in a weak acid (?a=1.6×10−5) and 0.510 M in its conjugate base, what…

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Q: The following solution mixture is/are buffer ... * O NaH2PO4 and Na2HPO4 O NH3 and (NH4)2SO4 HCOOH…

A: Buffer solution is made by mixing of weak acid and its salt with strong base or by mixing of weak…

Q: Predict what volume (mL) of 0.3000 M NaOH is required to titrate the 25.00 mL of 0.3000 M HCl to the…

A: The reaction can be written for the given information as follows, NaOH + HCl →NaCl + H2O

Q: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,),N), a weak base, and 0.20 M…

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Q: It took 32.47 mL of 0.1424 M NaOH to reach the endpoint when titrating a sample containing 0.615g of…

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Q: pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hint: How many moles of H+…

A: Given the volume of 1.0 M LiOH taken for titration = 20.0 mL  Volume of 0.20 M H2SO4 taken for…

Q: What is an acid–base indicator?

A: As per our guidelines,  you have posted multiple questions we can only answer first one.

Q: A 200 mL buffer solution is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX. Since…

A: A mixture of weak acid (HX)  and its salt (NaX) with strong base acts as acidic buffer solution. For…

Q: What is the pH at the equivalence point?

A: The balanced chemical equation for the above process is: NH3 + HCl ------------> NH4Cl We first…

Q: -> 100. ml OF 0. 200 M HCI is titrated with o. 250 M NaOH Question: What is the PH OF the solution…

A: Answewr:- This question is answered by using the simple concept of titration of strong acid against…

Q: Hard water + pH 10 buffer + EBT indicator, the mixture is?

A: Given information,       Hard water + buffer with pH 10 + EBT indicator

Q: A solution is prepared by mixing 80 mL of 0.2 M KH2PO4 and 120 mL of 0.2 M K2HPO4 . What is its pH?

A: Moles of KH2PO4 ( acid), = 0.2 M × 0.08 L = 0.016 mol   Moles of K2HPO4 (base), = 0.2 M × 0.120 L =…

Q: . What is the pH of the solution when 25 mL of 0.1 M HCl is titrated with 28 mL of 0.09M NaOH, pH =

A: pH can be calculated as follows

Q: Your facilitator asked you to prepare 450-mL of a buffer solution having a pH of 10.45 composed of…

A: The Answer to the following question is-

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: The K, for NH3 is 1.8 x 10-° at 25°C. Calculate the pH of a buffer solution made by mixing 45.7 mL…

A: Given data:- A buffer solution made by mixing 65.1 mL of 0.142 M NH3 with 38.0 mL of 0.172 M NH4Cl…

Q: In the laboratory, a general chemistry student measured the pH of a 0.528 M aqueous solution of…

A: Isoquinoline is a weak base pOH = 14 - pH pOH = -log [OH-] For a weak base: [OH-] = (Kb x C)1/2…

Q: A titration of 25.00 mL of sulfuric acid required 37.22 mL of 0.1124 M NaOH to reach the endpoint.…

A: Given; The molarity of NaOH, (M1) = 0.1124 M. The volume of NaOH, (V1) = 37.22 mL. The volume of…

Q: a) Fill in the blank: 1- The completion of the titration is detected by 2- PH + POH of acid-base…

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Q: Titration of 10.00 mL of a 0.444M solution of HCl with a solution of LiSH required 23.2 mL  of the…

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Q: Enough water was mixed with 1.26 g of sodium hydroxide (40.0 g/mol) to make a 500. mL solution. What…

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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.