M anserine buffered solution, pH 7.20. Answer the below questions: Volume of stock solution needed = ____ mL Volume of HCl needed to adjust the imidazole group = ____ mL Volume of HCl needed to titrate the
Q: 1. Calculate [H+], [OH-], pH and pOH of: a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4)
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Q: BUFFERS, HYDROLYSIS OF SALTS 1. A 0.0250 M Ca(X)2 has a pH of 8.049. Ca(X)₂ is composed of a Ca2+…
A: Given: The concentration of Ca(X)2 = 0.0250 M The pH of the solution of Ca(X)2 = 8.049 We have to…
Q: A Kapiolani Community College student titrated 250.0 mL of a 0.1000 M NaOH solution against a…
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Q: BUFFERS, HYDROLYSIS OF SALTS 1. A 0.0250 M Ca(X)₂ has a pH of 8.049. Ca(X)2 is composed of a Ca2+…
A: Note- Dear student, since the given question is a multipart question, hence I solved first question…
Q: A chemist titrates 160.0 mL of a 0.2739M trimethylamine ((CH, N solution with 0.4017M HCI solution…
A: To reach equivalence point, the required volume of the HCl is; MHCl×VHCl=MCH33N×VCH33NVHCl=160.0…
Q: enzoic acid (HBenz) has a Kvalue of 6.3 × 10-5. You need to prepare a buffer having a pH a of 4.05…
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Q: A chemist titrates 60.0mL of a 0.3452M benzoic acid HC6H5CO2 solution with 0.5460M KOH…
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Q: An analytical chemist is titrating 173.4 mL of a 0.6400 M solution of trimethylamine ((CH,) N with a…
A: When a strong acid is added to a weak base, then a buffer solution is formed. pOH of buffer solution…
Q: Consider a hypothetical diprotic acid (H2A) with pKa1 = 7.301 and pKa2 = 10.00. A 40.0-mL sample of…
A: GIVEN:- Consider a hypothetical diprotic acid (H2A) with pKa1 = 7.301 and pKa2 = 10.00. A40.0-mL…
Q: 1, Which of the following solutions is a buffer system? Group of answer choices 0.10 M HI and…
A: Equimolar amount of weak acid and its salt form buffer solution.
Q: A chemist titrates 240.0 mL of a 0.0766M ethylamine (C,H,NH, solution with 0.3238M HBr solution at…
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Q: A 1.00 L buffer solution is 0.050 M in HC7H5O2 and 0.200 M in LiC7H5O2. Calculate the pH of the…
A: Given: A 1.00 L buffer solution is 0.050 M in HC7H5O2 and 0.200 M in LiC7H5O2 The Ka for HC7H5O2 =…
Q: A chemist titrates 180.0 mL of a 0.8675 M trimethylamine ((CH3),N) solution with 0.4585 M HCl…
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Q: An analytical chemist is titrating 206.5 mL of a 0.9600M solution of cyanic acid (HCNO) with a…
A: Given- Volume of HCNO= 206.5 mL Concentration of HCNO= 0.9600M Concentration of KOH=1.100M Volume…
Q: The base ionization constant of ethylamine (C2H5NH2) in aqueous solution is Kb= 6.41 × 10-4 at 25°C.…
A: The reaction of Ethylamine when titrated with HCl is as follows:
Q: Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH =…
A: Stock solution of phosphate buffer of pH 6.5. Molarity of stock solution = 0.50M Ka= 6.32 ×10-8 We…
Q: Consider Titration of 50 mL of 0.20M H3A (Ka1= 8.2×10^-4 , Ka2= 2.9×10^-8 Ka3= 3.7×10^-11) titrated…
A: When a strong acid reacts with a strong base, then salt formation will happen and the reaction will…
Q: What volumes of equimolar aqueous solutions of K2HPO4 and KH2PO4 must she combine to make 600.0 mL…
A: In the aqueous solution, KH2PO4 will be dissociated to give a potassium ion and dihydrogen phosphate…
Q: A chemist titrates 60.0 mL of a 0.0919 M lidocaine (C4H,NONH) solution with 0.8547 M HBr solution at…
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Q: The phthalic acid is a diprotic acid (pKa1-2.95, pK₂2-5.41). A titration sample was prepared by…
A: mass of phthalic acid taken = 2.23 g Molar mass of phthalic acid = 166.14 g/mol => moles of…
Q: A chemist titrates 210.0 mL of a 0.1242M lidocaine (C₁4H21 NONH) solution with 0.6479M HBr solution…
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Q: Calculate the pI after 50 mL of 0.1 M NaI is titrated with 15.0 mL 0.2 M AgNO3 solution? Given (AgI…
A: Question is based on the concept of chemical equilibrium. We have to calculate p-value of iodide ion…
Q: Calculate the pI after 50 mL of 0.1 M Nal is titrated with 10.0 mL 0.2 M AgNO3 solution? Given (AgI…
A: Given the volume of 0.1 M NaI solution taken = 50 mL * (1L/1000 mL) = 0.050 L => moles of NaI…
Q: How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid…
A: Given: Molarity of NaOH = 0.120 M (i.e. mol/L) Molarity of hypochlorous acid [HOCl] = 0.0998 M (i.e.…
Q: Selected acid base/base pair: Propanic Acid (CH3CH2COOH) / Sodium Propanoate (NaCH3CH2COO) with Ka =…
A: Ka of propionic acid = 1.4 x 10-5 Propionic acid is weak acid and sodium propionate as conjugate…
Q: Harriet Rowki prepared 100.0 mL of 2.50 M HBO3-NaH2BO3 buffer solution (pH = 8.50). The pKa value of…
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Q: A 25.0 mL sample of a 0.1500 M solution of aqueous trimethylamine is titrated with a 0.1875 M…
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Q: 10. The normal pH of the stomach is around 3. A patient takes an antacid which raises the buffered…
A: In the problem the acidity levels of stomach, antacid and naproxen are around 5. so the solubility…
Q: 2. solution of diprotic acid with molar mass 186.0 g/mol (Ka1= 7.1e-2 Ka2=6.1e-5) made by placing…
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Q: A chemist titrates 170.0 mL of a 0.8630M lidocaine (CH21NONH) solution with 0.1298 M HNO, solution…
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Q: 1. When making a buffer of pH = 10, weak molecules with the following Ka values are available.…
A: Answer of 1&3 is given below, as in equation 2 there is not statement is given so answer is not…
Q: Consider a hypothetical triprotic weak acid H₃A, pKa1 = 4.00, pKa2 = 7.00 and pKa3 = 10.00 Which of…
A: Concepts to be used: Amphiprotic substances can either donate or accept proton (H+) based on the…
Q: An analytical chemist is titrating 179.6 mL of a 0.8400M solution of cyanic acid (HCNO) with a…
A: Given, Volume of HCNO = 179.6 mL Molarity of HCNO = 0.8400 M Molarity of KOH = 1.200 M Volume of…
Q: A buffer solution with pH = 5.0 is required, which one of the following acid, together with its…
A: The pH value of a buffer solution mainly depends upon the pKa value of the acid. If the pKa value of…
Q: A student needs to prepare a buffer made from HF and KF with pH 3.441. If Ka for HF is 7.20 x 10-4,…
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Q: Question 2 You mix together a buffer solution with 0.076 moles of HA and 0.078 moles of NaA which…
A: Buffer are solution which resist change in PH when acid Or base are added to the solution Here We…
Q: A chemist titrates 70.0mL of a 0.5352M carbonic acid (H2CO3) solution with 0.1825M KOH solution at…
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Q: CH3COOH+ NaOH The first titration used phenolphthalein, the endpoint was 43.5ml The second titration…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Starting with 0.0100 mol of KCN and the usual inorganic reagents of the laboratory, How would you…
A: Solution: Here we have 0.0100 mole of KCN. A conjugate strong base of HCN acid ( a weak acid). We…
Q: Calculate the pI after 50 mL of 0.1 M Nal is titrated with 20.0 mL 0.2 M AGNO, solution? Given (AgI…
A: Sodium iodide reacts with silver nitrate to give sodium nitrate and silver iodide. Sodium iodide…
Q: What is the pHpH of a buffer solution containing 0.20 MM HC2H3O2HC2H3O2 (acetic acid) and 0.20 MM…
A: Given :- [HC2H3O2] = 0.20 M [C2H3O2-] = 0.20 M Ka for acetic acid = 1.8 x 10-5 To calculate :-…
Q: The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H 2A…
A: The term that reflects any acid's potential or strength is specified as pKa. The stronger acids…
Q: Answer the following question about a titration between 25.0 mL of a weak acid (Ka= 6.2*10-5) and…
A: Given: Ka of weak acid = 6.2*10-5 Concentration of NaOH = 0.120 M pKa of resorcin blue ~ 5.3 pKa of…
Q: What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered…
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Q: A saturated solution of manganese(Ill) hydroxide was prepared, and an acid-base titration was…
A: The solubility product of salt is a constant at a given temperature irrespective of the source from…
Q: 1. Succinic/succinate buffer system can be used in experiments involving biological systems that…
A: Here we are required to find the mass of sodium succinate needed to prepare 2L of buffer
Q: Given: Ammonia (NH3(aq)) is a common component in cleaning agents. The ammonium cation (NH4+(aq))…
A: The pH value of any solution shows the characteristics of that solution. Any solution’snature…
Q: An aqueous solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka= 6.3 × 10-5for HC7H5O2.…
A: We have to find the pH
Q: Calculate the pHpH of the buffer that results from mixing 57.9 mLmL of a 0.278 MM solution of…
A: From given data M of acid HCHO2 = 0.278 V of acid = 57.9 mL= 0.0579 L M of salt NaCHO2 = 0.535 V of…
Q: How would you prepare 100.00 mL of 0.100 M phosphate buffer at pH 7.00 using solid KH2PO4 and…
A: Given data,Molarity of phosphate buffer=0.1MVolume of buffer=100mL=0.1LMolar mass of…
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- Calculate the phenolphthalein and total alkalinities of 300 ml sample that required 10 ml of 0.05N Hydrochloric acid to reach the phenolphthalein end point, and total of 15.5 ml to reach the methyl orange end point. What type of alkalinity is present? Express in mg/L.14. A so-called PBS buffer (phosphate buffered saline) is prepared by according to the given protocol: ● Prepare 800 mL of distilled water in a suitable container; ● Add 8 g of NaCl to the solution; Add 200 mg of KCl to the solution; Add 1.44 g of Na₂HPO4 to the solution; Add 245 mg of KH₂PO4 to the solution; Adjust solution to desired pH (typically pH ≈ 7.4); and Add distilled water until volume is 1 L. (a) Calculate the pH of the initial solution (before pH is adjusted). (b) How many moles of acid or base are required to adjust the pH to 7.4?A sample may contain NaOH, sodium carbonate and sodium bicarbonate, alone or in compatible combination. Titration of a 50.00 mL aliquot of the sample to a phenolphthalein end point required 8.50 mL of 0.0905 M HCl. A second 50.00 mL aliquot required 22.40 mL of the HCl when titrated to a methyl red end point. Calculate the molar concentration of the base component/s
- Calculate the pH of a solution prepared by mixing 1.50 g of imidazole with 1.50 g of imidazole hydrochloride and diluting to 100.0 mL. The pK, of imidazole hydrochloride is 6.993. pH = pH == 6.81 Incorrect Calculate the pH of the solution if 1.70 mL of 1.03 M HCIO, are added. 6,72 Incorrect volume: How many milliliters of 1.03 M HCIO, should be added to 1.50 g of imidazole to give a pH of 6.993? 6.73 Invert Curstinn San ml.What volume of 0.12 M HCl must be added to 1.5 g glycine amide to make buffer at pH 8.5? What volume of 0.08 M NaOH must be added to 1.1 g glycine amide hydrochloride to get a pH of 7.5?Suppose you want to make 250 mL 0.0700 M glycine buffer at pH 8.00. What mass of glycine amide and glycine amide HCl are needed? Hint: you need 2 eqns w/ 2 unknowns. Use the mb eqn and HH eqn. What mass of glycine amide and what volume of 0.400 M HCl are needed? What mass of glycine amide HCl and what volume of 0.600 M NaOH are needed?Imidazole (C3H4N2, FM 68.08) is a weak base with pKb = 7.01. You wish to make 250.0 mL of a 0.300 M buffer at pH 7.50. You can use one of two methods. a. First, starting with imidazole and imidazole hydrochloride, what mass of each would you need to combine and dilute to 250.0 mL to create your buffer? b. Now, starting instead with imidazole and 0.500 M HCl, what mass of imidazole should you use, and approximately how many milliliters of HCl will you need to add (before diluting to a final volume of 250.0 mL with water)? c. Of the two methods, which one is preferable and why?
- A solution contains compound X, which is a weak base, and its conjugate acid, in a molar ratio of weak base : conjugate acid = 1 : 5. The resulting solution has pH 5.26. Based on the Kö values below, which is compound X? NH₂OH Kb = 9.1 x 10-9 C5H5N Kb = 1.5 × 10-9 C9H7N Kb = 6.3 × 10-10 CoH5NH2 Kb = 4.0 × 10-10Given the following: citric acid pKa1 = 3.12, oxalic acid pKa1=1.25. Which of the following is true? a.Both acids can be used to buffer a solution at pH 4.0. b.The conjugate base of citric acid can be used as buffer at pH 8 c.Oxalic acid is a weaker acid than citric acid; d.The conjugate base of citric acid is more basic than the conjugate base of oxalic acid.Calculate the pH of a buffer solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield one liter of solution. The Ką of benzoic acid is 6.30 x 10-5 O 2.516 3.892 4.502 10.158 4.195
- a of m-chlorobenzoic acid, HC7H4CIO2, is 1.5x 10-4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC7H4CIO2 and 60.0 mL 0.1 M C7H4CIO₂ to give a final volume of 100.0 mL. What is the pH of this buffer? 4.0 (b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC7H4ClO2 and 40.0 mL 0.1 M C7H4CIO₂ to give a final volume 100.0 mL. What is the pH of this buffer? 4.0 (c) Why is buffer #2 more acidic than buffer #1? O It has a greater volume of base. O It has a greater final volume. O It was prepared after buffer #1. It has a higher acid concentration. -Suppose you are given solutions of 1.00 M acetic acid and 1.00 M sodium acetate and are asked to make 100.00 mL of buffer at pH 5.00 using only these two solutions. What volume, in milliliters, of acid would you need? The pKa of acetic acid is 4.75.: How would you prepare a liter of "carbonate buffer" at a pH of 10.10? H2CO3 > H* + HCO3 Ka = 4.2 x 10 HCO3 +> H* + co3 2 Ka = 4.8 x 10-11 13 buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution 2nobuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution 13 buffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1- L solution 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 solution