A certain indicator, HA, has a K, value of 5.0 x 10-7. The protonated form of the indicator is red and the ionized form is blue. What is the pK, of the indicator? 2 pK₁ = What is the color of this indicator in a solution with pH = 4? purple red blue

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Q: A certain weak base has a Kp of 7.30 x 10-7. What concentration of this base will produce a pH of…

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Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

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A: Answer: greater than 7

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Q: A 1.0-L buffer solution contains 0.300 mol acid, HA, and 0.300 mol base, NaA. The value of K, for…

A: Weak acid and its salt with strong base will make a buffer whose PH can  be calculated with the help…

Q: For the following, please answer all the questions. A 45.75-mL sample of a 0.125 M solution of…

A: Hey, since you have asked multiple question, we will solve the first question for you.  If you want…

Q: Which of the following is the correct definition of endpoint?     The point at which the indicator…

A: To solve this problem we have to know about Titration  and the term endpoint .

Q: What will be the pH of the buffer solution consisting of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189…

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Q: The indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is…

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Q: A solution is made by titrating 31.54 mL of 0.2315 M acetic acid (Ka = 1.74x10-5 M) with an equal…

A: 31.54 mL of 0.2315 M acetic acid31.54 mL of 0.2315 M KOHKa of acetic acid = 1.74×10-5

Q: A 10.0 mL solution of 0.360 M NH3 is titrated with a 0.120 M HCl solution. Calculate the pH after…

A: ( If you have any questions related to this problem please feel free to ask me).

Q: In pure water, what are the concentrations of H+ and OH- ions?

A: Given; ions

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A: The question is about calculating the pH of a buffer solution with the given data -

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Q: A solution is made with 554 ml of 8.21 M HX solution and 549 mL of 6.06 M Nax solution and the pH at…

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Q: Does the concentration of HC, H,0, increase or decrease when OH is added? O increase O decrease

A: NOTE- Since you've posted multiple questions, we are solving only the first question for you. If you…

Q: Name: NetID: 8. A titration is carried out where 50.0 mL of 0.300 M HF is titrated with a 0.190 M…

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Q: A 1.00 L solution contains 0.372 M HA (Ka = 2.93⋅10−62.93⋅10-6) and 0.741 M NaA.   What is the pH…

A: Here we are required to find the pH of the solution.

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A: pH range or buffer capacity of a buffer = pKa±1.

Q: In a titration of 77.0 mL of a 0.500 M solution of the diprotic acid H₂C₃H₂O₄ (malonic acid) with…

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Q: pH=pKa if the pH of the buffer solution contains equal concentrations of a weak acid and its…

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A: Using fundamental properties of buffer solution.

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…

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: Select the mixture which is capable of tolerating the addition of a strong acid without altering the…

A:

Q: What is the pH of buffer that is 0.175 M in a weak acid and 0.200 M in the acid's conjugate base?…

A: Given data, Molarity of weak acid=0.175MMolarity of conjugate base=0.200MKa=5.7×10-4

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: (The Ka value for HF is 6.6 x 10*.) 3. Using the value of K, from the previous question, show how to…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

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

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Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

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Q: aculate the pH after 0.02 mol of HCI is added to the buffer Which of the following is NOT an…

A: A conjugate base, within the Brønsted–Lowry acid–base theory, is a species formed by the removal of…

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.