1.Given the equilibrium for the indicator, HIn, below HIn (yellow) ⇌ H+ + In– (blue) pKa ≈ 3-4 What are the colors at the following pH? choose between blue, yellow green pH=2.88, pH=6.75, pH=4.78

Q: Bromothymol blue is yellow in acid solutions. HBB is acidic form of the indicator. The indicator is…

A: Acid will react with base and base will react with acid and carryout neutralization reaction.

Q: The indicator dinitrophenol is an acid with a Ka of 1.1 × 10−4. In a 1.0 × 10−4-M solution, it is…

A: The ionization constant expression gives the concentration of H3O+ ions which can further use for…

Q: A sample of nitric acid, HNO3 is titrated with NaOH. Which of the following would be the best…

A: This is a type strong acid vs strong base titration

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Answer: When a weak acid is added into water, it furnishes and these free ions conducts the…

Q: A 0.0200 M solution of a certain monoprotic weak acid is 18.0% ionized. What is the value of Ka for…

A:

Q: Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the…

A: Given,molarity of HC2H3O2 = 0.20 MVolume of HC2H3O2 = 20.0 mLMolarity of NaOH = 0.10 MVolume of NaOH…

Q: consisting

A: The neutralization reaction after the addition of strong base results into following changes-

Q: Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and…

A: Given information,    0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO)…

Q: If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.125 M, determine the carbonic…

A:

Q: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00250 M , determine the…

A: Given, H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq) pH of blood = 7.45 Acid dissociation constant (Ka) = 4.3 ×…

Q: What is the pH after 15.0 mL of 0.200 M HCl has been added to 100.0 mL of a buffer solution, X, with…

A: Given that,  Concentration of 100 mL weak base X solution = 0.70 M Moles of X in 100 mL buffer =…

Q: The ionization constant of a very weak acid, HA, is 4.0 × 10-7. Calculate the equilibrium…

A:

Q: Cyanohydric acid is a weak acid with Ka = 4 × 10-¹⁰. a) for 0.5 M hydrocyanic acid solution…

A:

Q: Consider an indicator that ionized as shown below for which its Ka = 1.0 x 10-4. HIn     +     H2O…

A:

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

A:

Q: What volume, in milliliters, of 0.240 M NaOH should be added to a 0.135 L solution of 0.030 M…

A: Here we have to determine the volume of 0.240M NaOH solution required to be added to 0.135L of…

Q: The following five beakers represent solutions of 5 different acids, at the same initial…

A: The acid dissociation constant (Ka) represents the strength of the acid. The higher the Ka the…

Q: Classify the following solutions as one of these types AND calculate the pH: strong acid, strong…

A: Given,a) 0.040 M NaF (Ka for HF = 7.2 x 10-4)b) 10 M HClO4c) A solution made by mixing 10.0 mL of…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Answer: When a weak acid is added into the water, its partial ionization takes place which causes…

Q: A certain indicator, HA, has a Ka value of 3.2×10−5. The protonated form of the indicator is red and…

A: pH indicates the existing quantity of hydronium ion in any provided solution. If the potential for…

Q: Bromothymol blue is yellow in acid solutions.  HBB is acidic form of the indicator . The indicator…

A: If we go on adding Sodium Hydroxide solution the Hydroxide Ion concentration will increase. this is…

Q: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the…

A: Concentration of bicarbonate ion required can be calculated using Henderson hasselbalch equation for…

Q: What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride?…

A: The solution can be easily determined using the Handerson HasselBach equation- pOH = pKb + log…

Q: What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN?  (Ka = 4.9 x 10-10…

A: Henderson - Hassel Balch Equation: The pH of the given buffer solution is given by Henderson -…

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

A: Given mixtures: 1.0 M NH3 and 1.0 M NaCl 1.0 M HCl and 1.0 M NaCl 1.0 M HNO2 and 1.0 M NaNO2 1.0 M…

Q: 9) The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the A of a weak acid she isolated called…

A: Answer: When a weak acid will be added in water, its partial ionization will take place, due to that…

Q: A patient presents itself to the emergency department in a critical condition. The patient’s blood…

A:

Q: Methyl orange is an indicator that changes color over a range from pH =3.1 to pH =4.4 . What is Ka…

A: Ka = 1.6 × 10-4

Q: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.0050 M, determine the…

A: pH is defined as the -ve log of the concentration of H+ pH = 7.35  -log[H+] = 7.35  log[H+] = -7.35…

Q: When a strong base is added to buffer it will react to become neutralized. Determine the pH after…

A: From the Henderson-Hasselbalch equation: Since, Ka = 5.8×10-10 Therefore,

Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

A:

Q: A certain indicator, HA has a Ka value of 6.3×10−8. The protonated form of the indicator is red and…

A: Given the Ka value of the indicator(HIn), Ka = 6.3*10-8  Color of the protonated forms(Hin) is red.…

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.