Q: What will be the pH
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Q: 2. If 25.00 mL of a 0.09864 M CH;COOH (Ka = 1.8 x 10-5) solution is titrated with a 0.1027 M NaOH…
A: At equivalence point only salt will be present
Q: Calculate how much you need to take from each solution to prepare 1 L of buffer solution with a pH…
A:
Q: A monoprotic weak acid has a Ka of 7.4 x 10^-6. What pH would a solution of 0.28 M of this acid…
A: The pH of a solution measures the acidity or basicity of a solution. If its value is more than 7,…
Q: A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL ot a buffer…
A: Buffer solution shows vary little variation or no change upon addition of an acid or a base.
Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…
A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…
Q: calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of a 0.100 M NaOH have been added to 40.0 mL of…
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: What is the resulting pH when 125 mL of a 0.1 mol/L CH3COOH solution is titrated with 75 mL of a 0.1…
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Q: 6- An indicator with acid dissociation constant (5.6×10-6), it's pH range will be ... 3.2-5.2…
A: Given: Acid dissociation constant of the indicator (KIn) = 5.6×10-6 We have to find the pH range of…
Q: Researchers have shown that hypochlorous acid (HCIO) generated by white blood cells kills bacteria.…
A: From Ka, α can easily be found. Then by multiplying the concentration with α, we can find the conc…
Q: A) 2.0 mL of 85% (w/w) concentrated H3PO4 (density 1.73 g/cm3) is diluted to 500 mL with water. What…
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Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH…
A: Buffer solutions are the solution which resist change in pH when small amount of acid or base is…
Q: It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3CO0 should be…
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Q: pH
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Q: What is the pH value of 0.085 M HNO2 (Ka: 4.5x10-4) and 0.1 M KNO2 solution?
A: Step : 1 What is the pH value of 0.085 M HNO2 (Ka: 4.5x10-4) and 0.1 M KNO2 solution?
Q: Describe, stepwise, how you would prepare 0.8 L of a 0.25 M phosphate buffer, pH 12.5, using…
A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…
Q: What is the pH of the solution when Caitlin has added 50.00 mL of the 0.25 M LIOH to the 25.00 mL of…
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Q: Answer the following with complete solution: How many grams of sodium formate, NaCHO 2 , would have…
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Q: 5) Calculate the volume of concentrated ammonia (molecular weight = 17) needed to prepare 100 ml of…
A: Given : Kb = 1.8 x 10-5 Density of solution = 0.9 g/ml Concentration of ammonia solution = 28%…
Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…
A: Given-> Volume of NH3 = 50.0 ml Molarity of NH3 = 0.15 M Volume of HCl = 15.0 ml Molarity of HCl…
Q: The pH value of 30 cm3 of a 0.2 M NaA solution is 9. What is the Ka of HA and the percent…
A: We have to calculate the Ka of HA and percentage ionization of HA.
Q: what is the pH of a solution that contains 0.75 M acetic acid (Ka= 1.8x10-5 ) and 0.50 Msodium…
A: Given data,Molarity of acetic acid=0.75MMolarity of sodium acetate=0.50MKa=1.8×10-5
Q: The pOH of 10 % titration of 10 mL of 0.10 M HCl with 0.10M NaOH is A 12.90 В 1.10 C) 10.0 D 7.00
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Q: n the titration of 20 mL CH3COOH (Ka = 1.76 x 10-5) 0.4 M with a solution of NaOH 0.4 M, calculate…
A: Since you have posted a question with multiple sub-parts, we will solve first three subpartsfor you.…
Q: The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H 2A…
A: Since the pKa1 will be represented by the point where the first equivalence point is reached And…
Q: How many grams of BHCl(acidic salt , 69.83g/mol
A: We have to find the mass of BHCl
Q: Calculate the pH of a mixture that contains 0.22 M of HCNO and 0.10 M of HC6H5O. The Ka of HCNO is…
A: Given : Concentration of HCNO = 0.22 M And concentration of HC6H5O = 0.10 M Ka of HCNO = 3.5 X 10-4…
Q: What is the pH when 50 ml 0.1 M NaOH is added to 50 ml the solution mixture of 0.1 M HA and 0.1 M…
A: pH can be calculated using the following equation: pH = - log (H+) pH of the solution is 3.65…
Q: Which weak acid would be best to use when preparing a buffer solution with a pH of 8.40? an acid…
A: Buffer solutions resist any changes in pH upon the addition of an acid or base to the solution. The…
Q: Using 0.1 M phosphate buffer, pH 7.2, prepare 25mL each of the buffer solutions with the following…
A: Given: 0.1 M phosphate buffer, pH 7.2, prepare 25mL eachof the buffer solutions with the following…
Q: Calculate the pH of a solution made by adding 0.11 g of solid NaOH to 275 mL of 0.250 M HNO2 (Ka =…
A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…
Q: Question attached
A: The pH value of the buffer solution is based on the pKa values of the acid When the pKa value of the…
Q: What is the pH of a solution made by adding 23.5 g of KC2H302 to 400 mL of 0.80 M HC2H302? (Ka for…
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Q: he pKa of the indicator is approximately 6, to which of the following equivalence point will it be…
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Q: A certain indicator, HA, has a K₂ value of 4.0 x 10-6. The protonated form of the indicator is red…
A: Given data : Ka=4.0×10-6pH=7 To find: pKa and color of indicator at pH 7
Q: What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and…
A: Ka = 1.8 × 10-5 pKa = - log Ka = - log (1.8 × 10-5) = 4.745.
Q: 3. Complete neutralization of 10 ml. of phosphoric acid solution by NaOH 0.I N in the presence of…
A: During titration of phosphoric acid we can use either methyl orange and detect first end point…
Q: 1.80x10-5) with 0.146 M NaOH. If the weak acid and NaOH reacts in 1:1 ratio, what is the pOH of the…
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Q: It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3COO should be…
A: Given;
Q: What is the pH of the solution that results from adding 25.0 mL of 0.012 M NaOH to 25.0 mL of 0.024…
A:
Q: How many grams of NaA (61.41 g/mol) would need to be added to 544 mL of 1.75 M HA to produce a…
A: Molarity of HA, [HA]=1.75 M Volume of the solution, V = 544 mL=0.544 L pH of the solution=5.49 Ka…
Q: 11-What is the pH of a solution obtained when 50 ml of 0.05 M NAOH is added to 100 ml of 0.05…
A: Since you have asked multiple question, we will solve the first question for you.If you want any…
Q: If a weak acid has a Ka of 2.04 x 10-7 what is the value of pKb?
A: Given Ka value of weak acid = 2.04 × 10-7 PKb = ?
Q: 3. Which indicator would show a pH change from 6 to 7? O Blue litmus indicator O Phenol red…
A: methyl red indicator
Q: A butanoic acid/sodium butanoate (C3H7COOH/NAOOCC3H7) buffer is prepared to 1.14x10-2 mol L-1…
A: pH = pKa + log(salt / acid) pKa = -log Ka
Q: Calculate [OH] in a solution obtained by adding 1.90 g solid KOH to 1.00 L of 10.0 M NH3. (Kb of NH3…
A: KOH is a strong base, whereas NH3 is a weak base.
Q: FRQ1: Consider the titration of 25.00 ml of 0.08 M of a weak acid, HA, with 0.125 M NAOH. Calculate…
A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…
Q: 2. A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 ml of solution…
A: Buffer solution :- A buffer solution is one which resists changes in pH when small quantities…
Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…
A: The acid ionization constant for lactic acid is 1.4×10 -4.
Q: The ion product constant of pure water at 40 °C with pH value of 6.77 is: O a 2.88 x 10-14 O b. 6.92…
A:
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- 5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3- Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2 Ka = 4.8 x 10-11 a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution d 2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solutionA sufficient quantity of each of the following aqueous solutions has been made available to you: (i) 0.2M NaH2PO4; (ii) 0.1M Na2HPO4 (a) How many ml of each of these two solutions would you require to mix together in order to prepare one litre of a 0.01M phosphate buffer pH 7.2? [For H3PO4: pKa1 = 2.15; pKa2 = 6.82; pKa3 = 12.38]. (Ans. = 14.7 ml 0.2M NaH2PO4; and 70.6 ml Na2HPO4). (b) Having calculated these volumes (of 0.2 M NaH2PO4 and 0.1M Na2HPO4) required, what further steps would you take to prepare the 0.01M phosphate buffer solution of pH 7.2?The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?
- ans asap In the use of EDTA as the complexometric titrant, at what pH value/s does Y4- become a major component of solutions? -At pH 1 -At pH 7 -At pH values lower than 10 -At pH values greater than 10The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.a. Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. b. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.1. To prepare 1 L of 0.10 M acetate buffer at pH 5.20, I need to mix g of CH3COONa (MW: 82.03 g/mol) with mL of 6.0 M HCl and dilute the solution to the volume of 1 L. (pKa of acetic acid is 4.76.) 2. If Lisa adds 50.0 mL of 0.060 M CH3COONa to 100.0 mL of 0.020 M HNO3 , what is the pH of the resulting solution?
- The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.H2PO4- + H2O <=====> HPO4-2 + H3O+ 1. Using 0.1 M phosphate buffer, pH 7.2, prepare 25mL each of the buffer solutions with the following concentrations at pH 7.2: a. 0.005 Mb. 0.05 Mc. 0.10 MA biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?
- Calculate the pH at the second stoichiometric point when 425 mL of 0.046 M solution of tartaric acid (Ka1 = 9.2E-4, Ka2 = 4.3E-5) is titrated with 1.00 M NaOH. a. The most suitable indicator for this titration would have pKIn closest to what value?4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .Please answer the following questions: 1. The phenolphthalein HIn indicator forms this equilibrium in an aqueous solution: HIn + H2O ↔ H3O+ + In-. During the course of titrating the acid content of samples, the concentration of H3O+ _________ , shifting the equilibrium towards _________ , until end-point is reached. a.decreases, In- b.increases, HIn c.decreases, HIn d.increases, In- 2. In the distillation of 70% isopropyl alcohol, which of the following is TRUE? a.The temperature was maintained at the boiling point of water. b.The 20 mL sample was distilled to dryness. c.The thermometer was allowed to touch the solution in the distilling flask. d.None of the above 3. Some Chem 16.1 students performed the ideal gas experiment on a hot summer day. Upon doing their experiment, the recorded temperature was 302 K.The pressure of the trapped air was found to be 763.0 torr. Given the following vapor pressures of water at certain temperatures, calculate the pressure of…