Buffers that are based on 3-morpholinopropanesulfonicacid (MOPS) are often used in RNA analysis. The useful pH range of a MOPS buffer is 6.5 to 7.9. Estimate the Kₐ of MOPS.
Q: Compute the buffer intensity, b, of a 10-1 M (= CT) acetic acid solution at pH 5 and pH 7. For each…
A: The pH of acetic acid solution is 5 and 7. The total buffer concentration of acetic acid solution is…
Q: A buffer is created by dissolving 0.303 moles of lactic acid and 0.197 moles of sodium lactate in…
A:
Q: In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation…
A: Buffer is a solution that resists the change in pH when small amount of acid or base to it.
Q: Calculate the molar solubility of lead(II) bromide (PbBr2). For lead(II) bromide, Ksp = 4.67 * 10 -…
A:
Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…
A: Henderson – Hasselbalch equation: It gives a relationship between the pka, pH, and concentration of…
Q: A buffer was prepared by adding 2.4 g ammonium nitrate to 100.0 mL 0.30 M ammonia (Kb = 1.8 x 10-5…
A: We have 2.4 g of ammonium nitrate , 100 ml of 0.3 M of ammonia, to this we added 10 ml of 0.3 M of…
Q: 27-29. Calculate the pH of the acetate buffer solution that contains 0.50M acetic acid…
A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…
Q: A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is…
A: According to Henderson-Hasselbalch equation,pH = pKa + log [conjugate base/acid]
Q: Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in !3! (1) pure water (2) pH = 2.00 buffer…
A: #1. Pure water: The equation for the dissociation of Ni(OH)2 is: Ni(OH)2(s) ⇌ Ni2+(aq) + 2OH-(aq)
Q: You are studying an unusual enzyme that produces hydronium ions (H3O+) during the course of the…
A: This question is from ionic equilibrium. We will figure out it answer with proper explanation.
Q: If NH4OH (aqueous ammonia, Kp = 1.8 x 10-5) is titrated with HCI, the pH at the equivalence %3D…
A:
Q: What must the ratio of acetic acid to acetate ion be to have a buffer with a pH value of 5.00?
A: acetic acid is weak acid Acetic acid ka =1.8×10-5 Salt of acetic acid is CH3COONa
Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…
A: Henderson equation for the calculation of pH of a buffer solution of a weak acid and strong base: pH…
Q: Determine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M…
A:
Q: A researcher in Biochemistry is isolating α-glucosidase enzyme from malted wheat flour. The protocol…
A: Given Values: The volume of lactate buffer needs to prepare = 2 Liter Concentration of the lactate…
Q: 3) A) Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…
A:
Q: A buffer consists of 0.25 M KHCO3 and 0.21 M K2CO3. Given that the K values for H2CO3 are, Ka1 = 4.5…
A: Given, 0.25 M KHCO3 0.21 M K2CO3 Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11
Q: . What is the pH of a buffer prepared by adding 0.405 mol of the weak acid HA to 0.507 mol of NaA in…
A:
Q: A mixture of ascorbic acid (CH706H, K2 = 6.8 X 105) and sodium ascorbate is prepared such that…
A:
Q: Calculate the pH of a carbonate buffer system that contains 0.0065 M HCO3 and 0.0084 M CO32-. The Ka…
A: The dissociation of HCO3- is as follows: By definition the Ka is,
Q: Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch…
A: Range for the target pH of a buffer solution that would favor pH stabilization using Henderson…
Q: A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…
A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…
Q: explain the importance of iodometric titration methods for the determination of iodine content in…
A: Iodometric titration method is used for the determination of iodine content in salt.
Q: In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation…
A: Buffers are solution that resists the change in pH when small amount of strong acid or base is added…
Q: A buffer is made by dissolving 21.5g of benzoic acid, HC7H5O2 (Ka = 6.4 x 10-4) and 37.7g of sodium…
A: Given: The Ka of benzoic acid = 6.4 × 10-4 We have to calculate the pH of a buffer made by…
Q: Report how to make 1.0L of an 0.25M, pH = 5.2 acetate buffer using glacial acetic acid and sodium…
A: A buffer solution is a solution whose pH remains unchanged upon addition of small amounts of acid or…
Q: cetic acid and a salt containing its conjugate base, such as sodium acetate, form buffer solutions…
A: Given that : Acetic acid and a salt containing its conjugate base, such as sodium acetate, form…
Q: You have a 258.3 mL sample of 1.659 M HA (Ka = 5.97⋅10−75.97⋅10-7). Calculate the pH of the best…
A:
Q: Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10-12) in a solution maintained at pH 9.00 and…
A:
Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…
A:
Q: Calculate the mas of KC2H3O2 that must be added to 500.0mL of a 0.200 M HC2H3O2 (Ka = 1.8 x 10-5)…
A: Given→ Volume of HC2H3O2 = 500.0 mL Molarity of HC2H3O2 = 0.200 M Ka…
Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.127 M solution…
A:
Q: h. The buffer capacity of buffer solutions is commonly defined by the pH range pKa - 1) to (pKa+ 1).…
A: Given pH range for buffer capacity of buffer solution pH = (pKa + 1) to (pKa - 1) pH given by…
Q: Calculate the molar solubility of Hg2C2O4(Ksp= 1.75 x 10-13) in 0.13 M Hg2(NO3)2.
A: The solubility reaction of Hg2C2O4 is => Hg2C2O4 (s) ------> Hg22+ (aq) + C2O42- (aq)
Q: What effect has a 1:10 times dilution of a buffer solution with pure water on its useful range or…
A: The Henderson-Hasselbalch equation for the pH of a buffer solution of the monoprotic acid is given…
Q: 9. Calculate the molar solubility of BaSO4 (Ksp = 1.1 x 1010) in %3D a. water. b. a solution…
A: The given data is as follows: The solubility product of BaSO4 = 1.1×10-10 The molar solubility of…
Q: Consider a buffer made by adding 52.3 g of (CH3),NH2I to 250.0mL of 1.42 M (CH3)¿NH (Kb = 5.4 x…
A: The concentration or Molarity of salt is calculated by - M = w×1000/m×V Here, M = Molarity of Salt,…
Q: A buffer solution consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5) and 0,35 mol∙dm–3…
A:
Q: A phenol/phenolate buffer was made up by mixing 0.0125 mol of phenol (C6H5OH) and 0.0135 m of…
A: Given : Moles of phenol = 0.0125 mol Moles of phenolate = 0.0135 mol Volume of buffer = 500 mL = 500…
Q: Consider the following buffer system: 1.03 M H3PO4 and 0.93 M H₂PO4-. What is the pH of such a…
A: Acidic buffer :- A mixture of weak acid and its salt with strong base is known as acidic buffer…
Q: What mass of sodium glycolate (98.03 g/mol) must be added to 300.0 mL of 1.00 M glycolic acid…
A: Given: pH of the buffer = 4.00 Ka of glycolic acid = 4.48×10-4 Molarity of glycolic = 1.00 M Volume…
Q: precipitation
A: There are various type of water softening operations but in them the Lime softening method is used
Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…
A: Given: pKa of lactic acid = 1.4 * 10-4
Q: You are asked to go into the lab and prepare an acetic acid -sodium acetate buffer solution with a…
A: The molar ratio of CH3COOH to CH3COONa has to be determined
Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…
A: Given, Concentration of propanoic acid = [CH3CH2COOH] = 0.1 mol/L Concentration of sodium propanoate…
Buffers that are based on 3-morpholinopropanesulfonicacid (MOPS) are often used in RNA analysis. The useful pH range of a MOPS buffer is 6.5 to 7.9. Estimate the Kₐ of MOPS.
Step by step
Solved in 2 steps with 1 images
- Explain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context of a titration.Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .At what point in the titration of a weak base with a strong acid is the maximum buffer capacity reached? This is the point at which a given small addition of acid causes the least pH change.
- What accounts for the discrepancy in pH? When you have already dissolved the computed masses of reagents for the buffer in an ample amount of distilled water, and upon checking the pH using the pH meter the pH is less than the target pH.What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.Acetic acid and a salt containing its conjugate base, such as sodium acetate, form buffer solutions that are effective in the pH range 3.7-5.7. (a) In resisting a pH change, which buffer component would react with NaOH? Explain. (b) What happens to the buffer activity when this component is exhausted?
- What effect has a 1:10 times dilution of a buffer solution with pure water on its useful range or its buffer capacity?Write the expression for the solubility constants of thefollowing compounds: (a) Agl, (b) Hg2S, (c) Fe(OH)3, (d) Ag2CrO4.Why might the actual pH of a prepared buffer deviate from its theoretical pH obtained using the Henderson-Hasselbalch equation? Give 4 examples of buffers in biological systems as well.
- Calculate the molar solubility of X(OH)3 within water. Ksp X(OH)3 = 8.3 x 10–34 2.6 x 10–9 M 1.7 x 10–17 M 2.4 x 10–9 M 6.0 x 10–19 M 2.9 x 10–17 MWhat is the relationship between the buffer range and the buffer-component concentration ratio?The weak base NH3 (concentration 0,10 mol∙dm–3) is titrated with strong acid HCl (concentration 0,050 mol∙dm–3). Without doing any calculations, explain why the pH at the equivalence point of this titration is less than 7.