A certain indicator, HA has a Ka value of 6.3×10−8. The protonated form of the indicator is red and the ionized form is yellow. What is the p?a of the indicator? p?a=     What is the color of this indicator in a solution with pH=5? red yellow orange

Q: What is the pH value of the final solution when 50 mL of a 0.5 M NaOH solution is added to 50 mL of…

A: Given: Volume of NaOH = 50 mL Molarity of NaOH = 0.5 M Volume of acetic acid = 50 mL Molarity of…

Q: A mixture needs to be separated to obtain pure individual components. One of the components is a…

A: For separation of mixture, we have to choose a perticular solvent that dissolve that particular…

Q: Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.13 mol NaOH is…

A: Given,Molarity of HF=0.60mol/LMolarity of KF=1.00mol/LMoles of NaOH=0.13 molMoles of HCl=0.26…

Q: Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF. The Ka for HF is 7.2×10-4. pH =

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

A: pH + pOH = 14 pH = -log[H+] pOH = -log[OH-] For a weak base solution: [OH-] = (kb × C)1/2 Given…

Q: is solution is prepared by mixing 25 mL of 0.1 M HCHO2 with 25 mL of .2 M NaCHO2. The pH of the…

A: Given values-> Volume of HCHO2 = 25ml Molarity of HCHO2 = 0.1 M Volume of NaCHO2 = 25 ml Molarity…

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

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Q: Which makes a buffer solution?   a weak acid + a weak base   b weak base + the salt of the weak base…

A: Buffer solution- buffer solutioh is  chemial solution is a chemical solution which consists of a…

Q: Which of the following pairs would make a buffer? O HNO3 and NO2 O KBr and HBr NH3 and NH4*CI NaCl…

A: buffer : it is a mixture that resist change of pH by adding small amount of buffer solution. buffer…

Q: monoprotic acid has a Ka of 1.50×10−4. Sketch the titration curve for a 50.0 mL 0.10 M sample of…

A: IMPORTANT POINTS  As dissociation constant given in the question is in the powers of 10-4 ,which is…

Q: A buffer solution is an aqueous solution consisting of a mixture of -- O a weak acid and its…

A: Buffer Solution is a water-based solution that consists of a mixture of a weak acid and its…

Q: Aniline, C6H5NH2₂, is a weak base that is commonly used in the preparation of precursors for…

A: we have to calculate  moles of aniline  volume of HCl at equivalence point  pH at the equivalence…

Q: Which of the following pairs of chemicals could be used to make a buffer solution? O NaC2H302 +…

A: Interpretation -  To tell about that which of the following pairs of chemical which could making a…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: In which of these solutions will the weak acid, HNO,, ionize less than it does in pure water? 0.15 M…

A: HNO2 is a weak acid. It dissociates as,  HNO2 ⇌ H+ + NO2- So, According to Le Chatelier's Principle,…

Q: What is the pH of the solution that results from mixing 25 mL of 2.30×102 M NH3 and 25 mL of…

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Q: A monoprotic acid has a Ka of 1.29×10−4. Sketch the titration curve for a 150.0 mL 0.050 M sample of…

A:

Q: When mixed in equal molar amounts, which of the following pairs of substances would create a buffer?…

A: The objective of the question is to identify which pair of substances, when mixed in equal molar…

Q: One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3).…

A: If the pH of the blood increases the buffer will act in such a way that reduces the pH. It is the…

Q: What is the concentration of conjugate base in a buffer that has a pH=6.39 and a Ka=4.66×10−5.…

A: Given that,  Concentration of [H+] in a buffer =4.07×10-7 M Ka value of weak acid = 4.66×10−5. Then,…

Q: If a colorless solution has [H3O+] of 7.25 x 10-2 M and thymol blue is added as an indicator, what…

A: Thymol blue is an indicator used in acid-base quantitative titration. In presence of acid it will…

Q: Which species make good standard solutions for acid-base neutralization titrations? sulfurous acid…

A: Concept introduction- Strong acid- is an acid which ionizes completely in water by loosing proton…

Q: You have 75.0 mL of 0.17 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka…

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Q: If a buffer solution is 0.160 M in a weak acid (Ka = 2.1 × 10-5) and 0.580 M in its conjugate base,…

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

Q: An analytical chemist is titrating 136.3 mL of a 0.1300M solution of ammonia (NH3) with a 0.1800M…

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

Q: In a titration of 80.0 mL of a 0.500 M solution of the diprotic acid H₂C3H₂O4 (malonic acid) with…

A: The balanced equation for the titration is H2C3H2O4(aq) + 2NaOH →Na2C3H2O4 (aq)+2 H2O(l)

Q: Given two buffer solutions:       Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO       Buffer 2 :…

A: The buffer solutions given are, Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO          Buffer 2 :…

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: You make 1.00 L of a buffered solution (pH solutions of each component of the buffered solution.…

A: A buffer solution can be made using a weak acid and the conjugate base of the weak acid. For…

Q: Predict whether the following aqueous solutions have a pH less than 7, very close to or equal to 7…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: 10. The normal pH of the stomach is around 3. A patient takes an antacid which raises the buffered…

A: In the problem the acidity levels of stomach, antacid and naproxen are around 5. so the solubility…

Q: Calculate the pH of a buffer prepared by adding 0.39 moles of ammonia and 0.44 moles of ammonium ion…

A: The mixture of ammonia and ammonium ion is a weak base and it's salt of strong acid respectively.…

Q: Calculate the pH of a solution at the equivalence point when 200.0 mL of a 0.20 M solution of Lactic…

A:

Q: 1. When 50.00ml of 1.000M HCl is titrated with 0.750M NaOH, the pH increases. What volume of NaOH is…

A: Titration is the process that helps to determine the concentration of a substance reacting in a…

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

A: A buffer solution contains a weak acid and its conjugate base.  The pH of a buffer solution can be…

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: 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: Buffer 2 will be 150 mL of 0.15 M Tris-HCl buffer with a pH of 8.5 Write out the chemical equation…

A: The objective of the question is to write out the chemical equation for a Tris-HCl buffer and…

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…

A:

Q: Which one of the following pairs of compounds would be able to function as a buffer? HBr and Br-…

A: *Acidic buffer is equimolar  mixture of weak acid and it's salt with strong base.  * HBr and HNO3…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 21.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁹)

A:

Q: Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH 4Cl with 200.0 mL of 0.32 M NH…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: A solution is made by mixing exactly 500 mL of 0.147 M NaOH with exactly 500 mL of 0.100 MCH3COOH.…

A:

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.