Consider the spectrophotometric pH measurement of seawater with the indicator thymol blue illustrated at the opening of this chapter. The blue form of the indicator In22 on page 202 has maximum absorbance at a wavelength of 596 nm (nanometers). The yellow form HIn2 has maximum absorbance at 435 nm. Measurements of absorbance at the two wavelengths allows us to find the ratio [In22]/[HIn2]. How would you use this measurement to find the pH?

Q: You plan to make a buffer solution with sulfurous acid (H₂SO3) and it undergoes dissociation…

A: To make a buffer solution at pH 7.040, we can use the Henderson-Hasselbalch equation: pH = pKa +…

Q: Indicators are usually weak acids and bases. Provide an educated guess based on your experiments…

A: Given : Indicators are usually weak acids and bases.

Q: Calculate the volume, in milliliters, of a 0.780 M KOH solution that should be added to 4.500 g of…

A:

Q: 10.00 mL sample of 1.20 M HNO2 (analyte) (pKa = 3.34 and Ka = 4.57x10-4) is titrated with 1.20 M…

A: Given , pka = 3.34 Molarity of HNO2 = 1.20 M Volume of HNO2 = 10 mL Mmol of HNO2 = M × V   = 1.20…

Q: What is meant by (i) a qualitative analysis; and (ii) a quantitative analysis? Give two examples of…

A: •QUANTITATIVE ANALYSIS:- Quantitative analysis means measurement of amount or data. It is…

Q: The pKa of hypochlorous acid is 7.530. A 52.0 mL solution of 0.114 M sodium hypochlorite (NaOCl) is…

A:

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

A: The balanced equation for the reaction of weak monoprotic acid, HA(Ka = 5.4*10-5) with NaOH(aq) is:…

Q: The indicator bromothymol blue is yellow in a solution whose pH is less than 6.0, green if the pH of…

A: Given--<>  [H3O+] = 3.45 ×10-3 M what is color of bromothymol blue = ?

Q: A certain indicator, HA, has a K, value of 5.0 x 10-7. The protonated form of the indicator is red…

A:

Q: The table below shows the plH values at which two different indicators change colour Indicator…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub- parts for…

Q: Calculate the volume, in milliliters, of 0.170 M NAOH that must be added to 315 mL 0.0547 M…

A:

Q: Calculate the pH of the mixture of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189 mol/L with 109 mL…

A:

Q: Calculate the pH and pOH of 306 mL of a phosphate buffer that is composed of 0.314 M HPO2 and 0.512…

A: = 0.314 M = 0.512 MKa = 4.50*10-13Volume of buffer = 306 ml

Q: A volume of 15.00 mL of NaOH was titrated to endpoint with 11.34 mL of 0.1311 M HCl. Calculate the…

A: Volume of NaoH =15 mL Volume of HCl=11.34 mL Molarity of HCl=0.1311M

Q: Calculate the PH of a solution made by mixing 50 ml of 0.3 M citrate monobasic with 25 mL of 0.2 M…

A: Citric acid has three acidic protons and dissociates in three stages, as represented by the…

Q: The solubility of CO2(g) in water at 25 °C and under a pressure of 1.00 atm is 1.45 g/L. If the air…

A:

Q: Calculate the pH when 27.2 mL of 0.13 M sodium hypochlorite is mixed with 32.4 mL of 0.214 M…

A: Given:  Volume of sodium hypochlorite = 27.2 mL Concentration of sodium hypochlorite= 0.13 M Volume…

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

A: Given data: Moles of acid=0.220 Acid is monoprotic which gives only one H+. HA→H+ + A- Ka = 5.1×10-5…

Q: Calculate the pH that results from the addition of 1.50 mL of an 0.0126 M aqueous solution of H2SO4…

A: Gram equivalence of sulphuric acid = 1.50 x 0.0126 x 2…

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

A: Answer:-This question is answered by using the simple concept of calculation of pH during the…

Q: 20.00 mL

A: mmoles of acid = ( 40.00mL • 0.100M ) = 4mmol  mmoles of base = ( 20.00mL • 0.100 M ) = 2mmol

Q: A 29.9 mL aliquot of arsenous acid that has a concentration of 0.688 M will be titrated with 0.337 M…

A: First to calculate the moles of each.  Then to calculate pH.

Q: Triprotic acid H3A has dissociation constants Ka1=4.5*10^-4, Ka2=1.1*10^-8, and Ka3 = 7.9*10^-11.…

A: GIVEN: Concentration of H3A= 0.100 M Volume of H3A= 60.00mL Concentration of KOH = 0.400 M Volume of…

Q: Give the name of another weak acid that will have a similar titration curve. Briefly explain the…

A: The given  titration curve is of volume  fumaric acid  vs volume of strong base and show two step…

Q: Prepare 1.73 L of a 0.85 M phosphate buffer with a pH of 6.67 using two reagents from the table…

A:

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 409 mL 0.0463 M…

A:

Q: water sample

A: Generally, drinking water has a pH of 7, which is neither acidic nor basic and is safe to drink. The…

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 353 mL 0.0443 M…

A: A buffer solution is a type of solution that resists changes in pH when small amounts of an acid or…

Q: Calculate the pH of the solution resulting from the addition of 95 mL of 0.48 M HCl to 49 mL of 0.31…

A:

Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: Given : Ka = 2 x 10-4  thymol orange is an acidic indicator.

Q: A solution was prepared with 0.318 mol of pyridinium fluoride (C,H,NHF) and enough water to make a…

A:

Q: what is the pH of 20.00mL 0.0350M H2SeO3 by 0.5M NaOH solution at titrant volumes 0mL 5mL 10mL 15mL…

A:

Q: Calculate the ph of a solution prepared by mixing 20mL of 0.25M h3po4 (ka1 = 7.11 x 10^-3, Ka2 =…

A: For H3PO4: moles H3PO4 = Molarity x Volume in liters = 0.25 M x 0.02 L = 0.005 moles Since H3PO4…

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

A: The question is based on the titrations.  We are titrating a weak acid with a strong base. We need…

Q: The glass electrode used in commercial pH meters gives an electrical response proportional to the…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

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

A: The question is based on the concept of titrations. we are reacting a weak acid and strong base. We…

Q: (a) Sodium acetate, CH3COONA was hydrolysed in water, H20. Show the reaction equations involved.…

A: Salt when undergoes hydrolysis reaction gives corresponding acid and base. Nature of resultant…

Q: The concentration of total phosphorous (HPO4^2- and H2PO4^-) found in a blood sample is determined…

A: Henderson - hasselbach equation enables the calculation of pH of a buffer solution made by mixing…

Q: Describe how would you prepare a "phosphate buffer" with a pH about 7.50. pka2 = 7.21 Na2HPO4 =1.99…

A: To check which of the following system of solution would given required buffer solution with pH =…

Q: Calculate the resulting pH of a solution made by mixing 45 mL of 0.42 M sodium carbonate with 41 mL…

A: A solution of a weak acid and its conjugate base acts as a buffer solution.Carbonate is the…

Q: Chromium(III) hydroxide is amphiprotic.   Write a balanced chemical equation showing how an…

A: Amphoteric substances are those which can react with acid as well as base. We have to write the…

Q: The solubility of CO2(g) in water at 25 °C and under a pressure of 1.00 atm is 1.45 g/L. If the air…

A: Air pressure is 1.00 atm. Pressure of CO2 in air =0.036100×1.00 atm=3.6×10-4 atm

Q: Describe 3 methods of pH determination.

A:

Q: Phenolphthalein works in the range pH 8 to 12.5 and turns pink in that range. What will occur if…

A: The indicators are chemical compounds that show changes in color at a definite change in pH. Hence,…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

A:

Q: Calculate the percent ionization of 0.0080 MM butanoic acid (Ka=1.5×10^−5).

A:

Q: Table 5. Drink mix concentrations and absorbances for constructing a standard curve [H3O+] (M)…

A: