2. Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and 12.70, respectively. 3. What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 104
Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…
A: Given that, Mass of formic acid = 0.3654 g Molecular mass of formic acid = 46.03 g/mol Volume of…
Q: Consider the titration of 20.0 mL of a sample of 0.105 M HC2H3O2 with 0.125M NaOH. (Ka = 1.8 x 10-5)…
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Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.75 M NH₄NO₃? Note that the base…
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Q: equivalence
A: ( M1 • V1 )NaOH = ( M2 • V2 )acid V1 = ( 0.15M • 25.0mL ) / 0.20M V1 = 18.75 mL Total volume,…
Q: A buffer solution contains 0.753 M KClO2 (Ka = 1.1 x 10-2) and 0.659 M HClO2. If 0.244 moles of NaOH…
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Q: Calculate the molarity of the acid (HA) and the conjugate base (A- ) . For acetate, use grams-to-mol…
A: (a)The molarity of conjugate base can be calculated as
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Q: What is the pH of a buffer that results when 5.46 mole of H3PO4 is mixed with 2.97 mole of NaOH and…
A: · Moles of H3PO4 = 5.46 mol· Moles NaOH = 2.97 mol· Volume of solution = 1.00 L· Ka1 = 7.5 × 10–3
Q: 1. A buffer solution is prepared by taking 0.25 moles of acetic acid (pKa = 4.76) and 0.400 moles of…
A: 1. Given,
Q: A 1.35 L buffer solution consists of 0.175 M butanoic acid and 0.336 M sodium butanoate. Calculate…
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Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…
A: Use Henderson Hesselbalch's equation to get the pH of buffer solution having weak acid and its salt…
Q: 4. Tris(hydroxymethyl)aminomethane [(HOCH2);CNH2–Tris, or THAM] is a weak base frequently used to…
A: 4. Solution - pH = pH is a scale used to specify the acidity or basicity of an aqueous solution.…
Q: What is the pH of 0.32 M acetic acid to 1.00 L of which 0.630 g of sodium acetate, NaCH, CO,, has…
A: Given :- [Acetic acid] = 0.32 M Mass of sodium acetate = 0.630 g Volume of solution = 1.00 L Ka…
Q: Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na.…
A: a. mol of acid = MV = 0.35*0.25 = 0.0875 mol of conjguate = MV = = 0.55*0.25 = 0.1375 after…
Q: A 0.386 g sample of propanoic acid (CH3CH,COOH, K, = 1.3. x 10) was dissolved to a final volume of…
A: Given that, Weight of propanoic acid = 0.386 g Molar mass of propanoic acid = 74.08 g/mol Moles of…
Q: 2.00 L of a buffer is prepared by combining 1000.0 mL of 0.500 M nitrous acid (HNO2 Ka = 7.1 x 10-4)…
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Q: How will you prepare a pH 4.50 acetic acid-acetate buffer such that when 1.00 mL of 10 M NaOH is…
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Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…
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Q: What is the pH of a buffer solution that is 0.50 M in formic acid (HCHO2) and 1.0 M in sodium…
A: The given problem can be solved by using Henderson-Hasselbalch equation given below as; pH=pKa + log…
Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…
A: Given: The concentration of acetic acid is 0.100M. The volume of acetic acid is 100 mL. The…
Q: Calculate the pH of a base buffer solution composed of 0.20 M NH3 and 0.15 M NH4Cl after the…
A: The formula to calculate the pH of the solution is, pOH+pH=14pH=14-pOH Given, The concentration of…
Q: If the concentration of the weak base ammonia is 0.10 M and it is titrated with 0.1 M HCl, and the…
A: In this question, we want to determine the pH of the Solution at Half way point ( also called half…
Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of formic acid (pKa=3.74) and 40.0…
A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…
Q: 1. Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells…
A: The Ka value of acetic acid is 1.8 × 10-5.pKa = -log(Ka) = -log(1.8 × 10-5) = 4.74.concentration of…
Q: What mass (in g) of sodium formate, HCOONa, must be added to 10.0 L of a 0.483 M aqueous solution of…
A: Here, we have to find the mass of sodium formate that must be added to 10.0 L of a 0.483 M aqueous…
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A: A buffer solution of 50Mm with a pH 6, has to be prepared using sodium succinate and disodium…
Q: The pK₂ value for HF is 3.14. Would a buffer prepared from HF and KF with a pH of 2.64 be considered…
A: Henderson-Hasselbalch equation is used for pH of a buffer solution. pH = pKa + log[conjugate…
Q: Determine the pH of a buffer solution consisting of 35.0g HC2H3O2 (MW = 60.06 g/mol) and 55.0g…
A: Given, mass of HC2H3O2 = 35.0 g Molar mass of HC2H3O2 = 60.06 g/mol mass of NaC2H3O2 = 55.0 g Molar…
Q: 1. How would you prepare 500.0 mI. of 0.050 M phosphate buffer solution, pH 6.7 from 0.20 M…
A: Way to prepare buffer using PH measurement we have given 500ml of 0.05M buffer will have 0.025mol of…
Q: Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is…
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
Q: 1- A sample weighing 1 g contains acetic acid (FW = 60 g/mol). The content of acetic acid in the…
A: Hello. There are multiple questions posted together. The first question has been solved. To receive…
Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.127 M solution…
A:
Q: You have 500.0 mL of a buffer solution containing 0.250 M acetic acid (CH₃COOH) and 0.240 M sodium…
A:
Q: suppose there is 1.00L of an aqueous buffer containing 600.0 moral & acetic acid (pk. 4.76) and 40.0…
A: NaOH is a base and when it is added to the buffer , it gets add up to the base concentration and…
Q: Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5. FW(propanoic acid) = 74.08 g/mol; FW(calcium…
A: Buffers are generally good over the range pH = pKa ± 1. For example, the acetate buffer would be…
Q: A 50.00 mL sample of ascorbic acid (H2C6H606) is titrated with 0.1200 M KOH. The second…
A: Here is your answer...... This curve is just for illustration of how titration takes place of the…
Q: 6. What is the pH of a mixture of 5 ml of 0.1 mol/litre sodium acetate and 4 ml of 0.1 mol/litre…
A: Solution: In this problem we will calculate pH using henderson equation.
Q: a) Calculate the pH of a buffer system made up of 0.25 M C6H5COOH and 0.35 M C6H5C00ONA. b)What is…
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Q: explain each of the following cases. a) when we treat 1 mol / liter of hydrochloric acid, the pH…
A: a) When we treat 1 M HCl with a base,at the beginning the pH increases but after certain time pH…
Q: Calculate the pH of a 0.2 M solution of NH2OH 2. Calculate the pH of a…
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine…
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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: Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.…
A: Given: [NH3]=0.50 M[NH4Cl]=0.20 MpKb=4.75Volume of solution=1.0 L To calculate: pH
Q: A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 M…
A: Given, A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and…
Q: Buffer solutions are used by the human body to maintain a constant pH for biochemical processes such…
A: Ka = 1.85 × 10-5 [ CH3COOH ] = 0.150 M [ CH3COO- ] = 0.150 M pKa = -logKa
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: Consider an 50.0 mL analyte solution containing 0.50 g of KHP, titrated against 0.10 M sodium…
A: Answer: This question is based on acid-base titration where acid is the analyte and base is the…
Q: 2) For the titration 100 mL of 0.1 M NH3 with 0.2 M HCI, what will be the pH of the solution after…
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Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…
A: 1- First calculate the concentration of NaClO : Using the Henderson equation, pH = pKa +…
Q: Calculate the amount of NaOH (in grams) to be added to 0.500 L of buffer equal to 1.00 M in acetic…
A: Hello. Since more than one question has been asked, the first question shall only be answered in…
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- Choose the acid below that would make the most effective buffer for a solution to maintain a pH of 5.00 (aq., 25 oC), given a 0.500 M concentration of it and its conjugate salt. a) propionic acid, Ka = 1.34 x 10–5 b) HN3, Ka = 1.90 x 10–5 c) butanoic acid, Ka = 1.52 x 10–5 d) NH4Cl, Ka = 5.56 x 10–10 e) benzoic acid, Ka = 6.30 x 10–5Given the Kb's of three weak bases and the Ka's of two weak acids choose the one that could be used as one of the components of a buffer solution with a pH of 6.35. 1. CH3COOH (Ka = 1.8 x 10–5) 2. NH2OH (Kb = 1.1 x 10–8) 3. CH3NH2 (Kb = 4.4 x 10–4) 4. C5H5N (Kb = 1.7 x 10–9) 5. HCOOH (Ka = 1.8 x 10–4)A buffered solution containing disolved aniline, C6H5NH2, and aniline hydrochloride, C6H3NH3Cl, has a ph of 5.71 A. determine the concentration of C6H5NH3+ in the solution if the concentration of C6H5NH2 is 0.290 M. The pKb of aniline is 9.13 C6H5NH3+ = M B. Calculate the change in pH of the solution (delta)pH, if 0.377 g NaOH is added to the buffer for a final volume of 1.05L. assume that any contribution of NaOH to the bolume is negligible (delta)pH =
- 2. Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and 12.70, respectively. 3. What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 104 4. Tris(hydroxymethyl)aminomethane [(HOCH2);CNH2–Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kp is 1.2 x 10-6 and pKå is 5.92. The corresponding pKą is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer? 5. Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4CI. Calculate the pH change that takes place when a 100-mL portion of (A) 0.0500 M NaOH and (B) 0.0500 M HCİ is added to 400 mL of the buffer solution. Kb = 1.75 x 10s2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?
- An analytical chemist is titrating 161.4 mL of a 0.8000M solution of trimethylamine ((CH,) N) with a 0.8900M solution of HIO3. The p K, of trimethylamine 3 is 4.19. Calculate the pH of the base solution after the chemist has added 161.5 mL of the HIO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places.4. How many grams of sodium lactate, NaC3H5O3, should be added to 1.0OL of 0.150M lactic acid, HC3H5O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. Ka of lactic acid is 1.40 x 104.ebinolra muinonmA chemistry graduate student is given 250. ml. of a 0.80 M diethylamine (C2H5)2NH2Br solution. Diethylamine-3 is a weak base with K, = 1.3 x 10 • What mass of (C2H5)2NH2Br should the student dissolve in the (C2H5)2NH solution to turn it into a buffer with pH = 10.92? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
- Calculating the pH of å Weak Base lilla An analytical chemist is titrating 61.7 mL of a 0.3400M solution of aniline (CH,NH, with a 0.8400M solution of HIO3. The p K, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 10.9 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. dh pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility 24 MacBook AirAn analytical chemist is titrating 139.4 mL of a 0.7600M solution of isopropylamine ((CH3)2CHNH₂) with a 0.2500M solution of HNO3. The p K of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 308.2 mL of the HNO3 solution to it. ? Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X Ś 000 18 Arsuppose we drop (10ml of 1 M) of strong base (NaOH) into our buffer. Calculate the PH value for this buffer if the concentration of acetic acid [CH3COOH]=0.09M, and the concentration of [CH3CO0-]=0.11M.(Pka =4.74) снзсоон +он эснзсоо-+ Н20 5.21 O 4.22 3.11 O 4.92 O