Which indicator would be most appropriate for the titration of ammonia (pKa=9.3) and HCl? The answer is Phenol red, but why?

Q: In a titration of 47.0 mL of a 0.750 M solution of a triprotic acid H3C6H5O7 (citric acid) with…

A:

Q: A diprotic acid is titrated with a strong base. The pH at the first half-equivalence point is…

A: During the acid-base titration where weak acid is the analyte and strong base is the titrant and as…

Q: Discuss the structure and function of ion channels and describe their importance in medicinal…

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

Q: A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is…

A: NaOH is a strong acid, so first it will be completely neutralised by the strong acid HCl. The…

Q: 40 mL of NaOH solution with unknown concentration is titrated with 0.10 M of CH3COOH solution in the…

A: From the given data we haveVolume of NaOH (V1)=40mlMolarity of NaOH (M1)=?Volume of…

Q: Calculate the pH at the equivalence point for the following titration: 0.25 M HCl versus 0.25 M…

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Q: Consider the titration of 16.0 mL of 0.100 HCN with 0.200 M KOH. When 7.0 mL of titrant is added,…

A: Given : concentration of HCN and KOH. To find : either statement is True or false. Solution : As we…

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A:

Q: calculate the pH at the equivalence point for the following titration: 0.01M HCl versus 0.01 M…

A: Given,Molarity of HCl = 0.01 MMolarity of CH3NH2 = 0.01 MKa of CH3NH3+ = 2.3 x 10-11

Q: If 24.8 mL of 0.107 M acid with a pKa of 5.76 is titrated with 0.102 M NaOH solution, what is the pH…

A: pH = pKa + log [salt]/[acid] Number of moles = molarity x volume (L)

Q: Assume that 32.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a…

A: Acid and base react with each other to form salt and water. The nature of salt depends on the nature…

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is…

A: Given data,[HA]=0.2M[A-]=0.1MpKa=7.5Molarity of KOH=1MVolume of KOH=50mL0.05LVolume of buffer=1L

Q: Solution containing 2.00 mol of Ca(OH)2 is titrated with HCl. How many moles of HCl are required to…

A: We have to predict the moles of HCl required.

Q: Determine the pH of a buffer that is 0.55 M HNO₂ and 0.75 M KNO₂. The value of Ka for HNO₂ is 6.8 ×…

A: Acid & its salt forms acidic buffer.

Q: Each graph below represents a titration involving solutions of two of the following substances: HCl,…

A: HCl vrs KOH graph is D  HNO2 vrs KOH graph is B HCl vrs NH4OH graph is C  HNO2 vrs NH4OH graph

Q: In a titration of 52.0 mL of a 0.400 M solution of a diprotic acid H₂C₂O₄･2H₂O (oxalic acid…

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Q: What is the pH of a buffer solution that is 0.159 M in hypochlorous acid (HCIO) and 0.121 M in…

A: Given: Concentration of hypochlorous acid (HCIO)=0.159 M Concentration of  sodium hypochlorite…

Q: You are working in a lab and someone has just handed you a beaker filled with 110 ml of a mysterious…

A: pH of a buffer is calculated using Hasselbach Henderson equation: pH =pKa+log([Conjugate…

Q: If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,10…

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Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has…

A:

Q: What is the pH of the resulting buffer solution when 25mls of 0.10 M NaH is added to 25mls of 0.200…

A: pH of the buffer solution is calculated by using Henderson equation, it is,

Q: A certain indicator, HA, has a K, value of 1.0 × 10-5. The protonated form of the indicator is red…

A: pKa = -log Ka pH = -log[H+]

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A: Answer :-               pH = 1.845…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: Which of the following titrations result in an acidic solution at the equivalence point?…

A: Answer -  Equivalence point - The equivalence point  is the point in a chemical reaction when there…

Q: In the titration of 100.0 mL of 0.050 M CH3COOH (pKa = 4.74) solution, what will be the pH after…

A: Given,  The titration of 100.0 mL of 0.050 M CH3COOH (pKa = 4.74) with 10.0 mL of a 0.10 M NaOH…

Q: Consider a beaker containing 50 mL of 0.20 M of a weak acid (HA) with a pKa of 5.25.    How many…

A: Henderson equation is pH = pKa + log [salt][acid] when NaOH is added to weak acid then they react to…

Q: Enter your answer in the provided box. Calculate the pH of a bicarbonate/carbonate buffer in which…

A:

Q: the titration of 100.0 mL of 0.050 M CH3COOH (pKa = 4.74) solution, what will be the pH after adding…

A:

Q: If you were trying to prepare a buffer with ammonia, NH3, what would be the substance that you would…

A: 1. Buffer solution are those whose pH value doesn't chage appricableby addition of small of acid…

Q: In a titration of 68.0 mL of a 0.750 M solution of a triprotic acid H₃C₆H₅O₇ (citric acid) with…

A: Given that -  Volume of triprotic acid, citric acid , H₃C₆H₅O₇  = 68.0 mL  Molarity of citric acid,…

Q: The acid HZ has a pKa of 7.03.  If 25.00 mL of a 0.111 M solution of HZ are titrated with 0.100 M…

A: The objective of the question is to determine the pH before the addition of any base.It is given…

Q: If 26.7 mL of 0.106 M acid with a pK₂ of 5.37 is titrated with 0.102 M NaOH solution, what is the pH…

A: Please find your solution below : Acid-base titration is a method of qualitative analysis in which…

Q: A certain indicator, HA, has a K value of 0.00025. The protonated form of the indicator is blue and…

A: • The values provided in the question are:-  i) Ka value of a certain indicator HA = 0.00025    •…

Q: A titration curve is constructed by titrating 50.0 mL of 0.100 M solution of a weak acid, HA, with…

A:

Q: In a titration of 34.0 mL of a 0.250 M solution of a triprotic acid H3PO4 (phosphoric acid) with…

A: The question is based on the concept of titrations. We are titrating a weak triprotic acid with a…

Q: Which of the following pairs would pe appropriate to make a buffer of pH 3.0? O H2SO3 and NaHSO3 O…

A: If a weak acid pKa lie between the buffer zone then weak acid and it's salt act as a good buffer.…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 101º)

A: HCN=acid NaCN =salt Buffer solution A buffer is a solution can ability to resist pH change upon the…

Q: If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,050…

A: Given data, Molarity of NH3=0.10mol/dm3=0.10mol/LVolume of NH3=25.0cm3=0.025LMolarity of…

Q: Which conjugate acid-base pair would be the best choice when preparing a buffer of pH 5.23?

A: An acidic buffer is a solution of a weak acid and a salt.As the name suggests, these solutions are…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK, = 4.20)…

A: Given,  Volume of the buffer solution = 100.0 mL  pH = 4.00  [Benzoic acid] = 0.100 M  [Sodium…

Q: Calculate the pH at the equivalence point for the titration of 0.200 M methylamine (CH3NH2) with…

A: CH3NH3+ →CH3NH2 + H+ Ka =  [CH3NH2] [H+][CH3NH3+] Given that,Kb = 5x10-4 Ka x Kb = Kw Ka =…

Q: If the pKa for formic acid is 3.75 the ratio of formate (A) to formic acid (HA) at pH 4.15 is 5:1.…

A: Since you have posted a question with multiple subparts , we will solve the first three subparts for…

Q: The half‑equivalence point of a titration occurs half way to the equivalence point, where half of…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

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.