Q: Calculate the pH of a solution containing 0.0460 M potassium hydrogen tartrate and 0.028 M…
A:
Q: Buffers that are based on 3-morpholinopropanesulfonicacid (MOPS) are often used in RNA analysis. The…
A: The pH range of the buffer solution is 6.5 to 7.9 The pKa value gives us the idea of the acidic…
Q: The pKb of the organic base nicotine (denoted Nic) is 5.98. Write the corresponding protonation…
A:
Q: In solution, fentanyl is most stable in the pH range 3.5-7.5. What mass of acetic acid and sodium…
A: Solution- Data given- volume is 1 L, concentration is 30 mM, molecular mass (RMM) of acetic acid…
Q: 1.Calculate the change in ph when 5ml of 1M HCl solution is added to 1L of 100mM Tris solution at ph…
A:
Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0651 M HNO3 to…
A: The balanced equation is C2H5N + HNO3 -------> C2H5NH+NO3– Number of moles of C2H5N = M*V =…
Q: 5. Estimate the concentration of Ethanoic acid of a buffer solution containing 16.4 g/L CH3COONa and…
A:
Q: A group of students were able to isolate a novel amylase from the saliva of a pig found in Country…
A: Given the desired pH = 7.4 We can find the most suitable buffer based on the Henderson equation.
Q: Calculate the molar solubility of Ni(OH)2 (Ksp = 2.0 × 10-15) in a solution which is buffered at pH…
A: Ksp of Ni(OH)2 = 2.0×10-15 pH = 9.75 Using relation: pH + pOH = 14 pOH = 14 - pH = 14 - 9.75 =…
Q: A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and…
A:
Q: ACID-BASE EQUILIBRIA AND SALT EQUILIBRIA (COMMON-ION EFFECT, BUFFER AND SOLUBILITY EQUILIBRIA) A…
A: The mixture of Acetic acid and sodium acetate will form acidic buffer solution Give that…
Q: What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid…
A: We have to predict the pH of buffer solution.
Q: If 24.8 mL of 0.107 M acid with a pKa of 5.76 is titrated with 0.102 M NaOH solution, what is the pH…
A: pH = pKa + log [salt]/[acid] Number of moles = molarity x volume (L)
Q: 500ml of a 0.1M sodium phosphate buffer with pka of 7.21is diluted. Calculate the pH of of the…
A:
Q: A 20 ml solution of 0.1 M glycine hydrochloride has been prepared. How many moles of the weak acid…
A: Given, Molarity of glycine hydrochloride (say HA) = 0.1 M Volume of glycine hydrochloride = 20 mL…
Q: The Ksp for nickel(II) hydroxide at 25 degrees Celsius is 2.0 * 10^-14. What is the molar solubility…
A: Given that: Solubility product constant (Ksp) of Ni(OH)2 = 2.0×10-14 pH = 10.102 At 25°C pH + pOH =…
Q: A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if…
A: The given data contains, Acetic acid = 0.15 M. Sodium acetate = 0.34 M. pKa of acetic acid = 4.87
Q: A litre of solution containing 0 1 mole of CH3COOH and 0.1 mole of CH3COONa provide a buffer of PH…
A: Given , Moles of CH3COOH = 0.1 mol Moles of CH3COONa = 0.1 mol pH of the buffer = 4.74 Moles of NaOH…
Q: The base ephedrine has a pKa value of 9.6. Calculate the theoretical end point pH when a 0.1 M…
A: Ephedrine, the organic molecule used in the prevention of low blood pressure and asthma. The…
Q: Given the identity of the base, its concentration and pKb, determine the pH of a solution of the…
A: Whenever a weak acid and strong base reacts with each other than they form a weak acid strong base…
Q: Consider the titration of 50.00 ml of a solution of 0.2574 M of the fully protonated form of the…
A: Determine the number of moles. Number of moles of glycine = Molarity (M) × Volume (L)…
Q: The Ka of bromoacetic acid is 2.00 ×10–3. What masses of bromoacetic acid (CH2BrCOOH) and sodium…
A:
Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7. The…
A: Since, Ka of NaHCO3 = 4.8 × 10- So, pKa = -logKa = -log (4.8 × 10-11 ) = 10.32 The ratio of…
Q: Which conjugate acid/base pair could be used to create a pH 3.20 buffer solution with the largest…
A: Buffer works well when - pH = pKa Ratio of [Conjugate base] / [Acid] = 1:1
Q: What is the ratio of the concentration of acetic acid and acetate ions required to prepare a buffer…
A:
Q: Calculate the pH at which pilocarpine (basic drug) starts to precipitate from a 2% w/v aqueous…
A: Solution- poOH=pKb + logConjugated acidbasegivehn pKa of pilocarpine…
Q: The alkalinity of verde river is 250mg CaCo3/L. Calculate the molar concentration of the following…
A: Alkalinity refers to the ability of a solution to react and neutralize the acids in the water.…
Q: There are many organic acids and bases in our cells, and their presence modifies the pH of the…
A: Henderson Hasselbalch equation: Ka is the acid dissociation constant. Given data: Acid is lactic…
Q: A student needs to prepare a buffer solution with a pH of 5.26. Assuming a pKa of 4.73, how many mL…
A: A buffer solution is the one which is formed by mixing “a weak acid with the solution of the salt of…
Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…
A: Given data, Ka for NH4+=2.0×10-5Kf for [Ni(H2O)5(NH3)]2+=501
Q: Calculate the change in pH when 5.8 mL of 1.6 M NaOH are added to 100. mL of buffer solution in…
A:
Q: The pH of a solution containing 0.010 M lactic acid and 0.087 M lactate is 4.80. Calculate the pKa…
A: Given:Concentration of lactic acid = 0.010 M Concentration of lactate = 0.087 M pH of the solution…
Q: 1. Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is…
A: Given, 1.A buffer solution containing an acid with a pKa is 2.3 and an acid concentration is…
Q: A 100.0 mL solution containing 0.973 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.364 M…
A:
Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7. The…
A:
Q: Acetic acid (pKa = 4.75) is contained in vinegar. 1. Calculate the pH of an 0.1500 M aqueous…
A: As per our guidelines, we can only solve one question at a time. Please post other questions as next…
Q: Aniline, C6H7N (molar mass = 93.13 g/mol), is a weak base that is used as a precursor in the…
A: 924 mg of aniline is dissolved in enough water to make a total volume of 1.00 L. pKb of aniline…
Q: Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is…
A: A solution which resists change in pH when a small amount of acid or base is added to it is known as…
Q: The pKa of a weak acid was determined by measuring the pH of a solution containing the weak acid at…
A:
Q: Sketch a titration curve for the amino acid cysteine, and indicate the pKa values for all titratable…
A: Cysteine is a polar uncharged amino acid containing a thiol group (SH), which on reaction with thiol…
Q: What is the pH when preparing a solution od 1 mol NaOH and 2 mol of solid NaH2PO4? The pKa's of…
A: Given: Moles of NaOH = 1 mol. Moles of NaH2PO4 = 2 mol.
Q: calculate the ph of a 0.465 M solUTION OF ethylamine CH3CH2NH2 and 0.211 M ethylammonium bromide…
A:
Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7. The…
A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…
Q: How many moles of sodium acetate must be added to 500 mL of 0.25 M acetic acid solution to produce a…
A:
Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.89. The…
A: Answer is explained below. The given information are as follows:
Q: Aniline, C6H7N (molar mass = 93.13 g/mol), is a weak base that is used as a precursor in the…
A: The solution is given below -
Q: What weight of Na2HPO4 and H2PO4 would be required to prepare 200mL of a buffer solution of pH 7.40…
A: Given data, Na2HPO4 and H2PO4 prepared 200mL of a buffer solution of pH 7.40 Ionic strength =…
Q: what is the pKa of the acid?
A: Given :- pH of solution = 4.9 Concentration of conjugate base = x Concentration of acid = 2.3 x…
Q: Please answer 13.3 and 13.4
A:
A mixture of 0.20M ethanoic acid and 0.30M sodium acetate is given. What is the pH of the medium if the pKa of ethanoic acid is 4.76?
Step by step
Solved in 2 steps with 1 images
- The primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set at 7.4, what is the ratio of the concentrations of carbonate to bicarbonate. Describe the buffering capacity of this buffer.If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,10 mol∙dm–3), calculate the pH at the equivalence point of the titrationExplain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context of a titration.
- Calculate the molar solubility of Ni(OH)2 when buffered at pH 10.0 ?What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pK a of the acid is 5.7.ACID-BASE EQUILIBRIA AND SALT EQUILIBRIA (COMMON-ION EFFECT, BUFFER AND SOLUBILITY EQUILIBRIA) A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if the pKa of the acetic acid is 4. 87.
- What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?Determine the pH at the equivalence (stoichiometric) point in the titration of 38.83 mL of 0.262 M (CH3)2NH(aq) with 0.111 M HCl(aq). The Kb of (CH3)2NH is 5.4 x 10-4.You are asked to go into the lab and prepare an acetic acid – sodium acetate buffer solution with a pH of 4.00. What molar ratio of sodium acetate (CH3COONa) to acetic acid (CH3COOH) should be used? The pKa for acetic acid is 4.74
- Discuss the titration curve (variation of pH with respect to addition oftitrant) with suitable diagram and reactions involved when potassiumhydroxide (KOH) a strong base is added as titrant to acetic acid(CH3COOH) a weak acid analyte.Define and explain the significance of the equivalence point of a titration. Identify the role of the indicator in this context.Determine the pH at the equivalence (stoichiometric) point in the titration of 44.27 mL of 0.138 M morphine(aq) with 0.271 M HCl(aq). The Kb of morphine is 1.6 x 10-6.