III). You mix 100.0 mL of 0.20 M NaCH3CO0 with 20.00 mL of 0.200 M HCI. Calculate the pH of the mixture. The total volume is 120.0 mL. K, of CH;COOH = 1.8 x 10-5.
Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…
A: pH of solution can be found using the henderson-hesselbech equation.
Q: What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 20.00 mL of 0.10 M…
A: Given, NH3= 20mL of 0.1M Kb= 1.8× 10-5 NH3 = Weak base NH4Cl = Salt This is a buffer solution…
Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…
A: Answer:- Henderson-Hasselbach equation :- This equation is used for the determination of pH or pOH…
Q: A solution is generated by combining 50.0ml of 0.310M nitric acid (Ka=2.4x10^1) with 50.0ml of…
A: Solution : While determining the pH of the solution which is generated by combining strong acid…
Q: A solution contains 0.08 M acetic acid, HC 2 H 30 2 (K a = 1.7 × 10 -5 at 25°C) and 0.15 M sodium…
A:
Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…
A:
Q: a) A student mixed 200 mL of 0.15 M ammonium chloride, NHẠCI with 200 mL of 0.23 M ammonia solution,…
A: Kb for NH3 = 1.8 × 10–5 Ka for NH4+ = 1×10–14/Kb =1×10–14/(1.8 × 10–5 ) = 5.56 × 10–10 The solution…
Q: If a buffer solution is 0.170 M in a weak base (Kb = 4.2 × 10-5) and 0.490 M in its conjugate acid,…
A: Buffer solution: It is an aqueous solution which contains a mixture of a weak base and its conjugate…
Q: What is the pH of a solution prepared by mixing 18.00 mL of 0.277M CH3COOH with 50.00 mL of 0.166 M…
A:
Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,l? (Kb of CH;NH, is 4.4 x…
A: This is a basic buffer solution. A buffer resist the change in PH of the solution.
Q: Calculate the pH of a solution prepared by mixing 15.0 mL of .100 M NaOH and 30 mL of .100 M benzoic…
A: The moles of given acid and base can be calculated as
Q: The weak base dimethylamine, NH(CH3)2, has a molar mass of 45.09g/mol and a base-dissociation…
A: pH is used to measures the concentration of hydrogen ion. The expression for calculating the pH is…
Q: Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and…
A: We will calculate pH
Q: Calculate the mass of solid NaCH3CO0 that must be added to 1.0 liter of 0.20 M CH3COOH solution so…
A:
Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…
A: pH = 12.155 Therefore, pOH = 14 – 12.155 pOH = 1.845 So,as we know that ; [OH¯] = 10¯pOH =…
Q: An aqueous solution contains a mixture of 0.0500 M HCOOH (K, = 1.77 × 10-4) and 0.150 M CH;CH,COOH…
A: From the reaction: Initial 0.0500 M 0 0 Change +(x+y) +x Equilibrium (0.0500-x) (x+y) x…
Q: I mix 50.0 mL of 0.150 M CH3COOH with 10.0 mL of 0.100 M NaOH. Calculate the pH of the mixture.…
A: Henderson equation: pH = pKa + log[CH3COONa]/[CH3COOH] pKa = -logKa
Q: What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of…
A:
Q: 1. Calculate the pH of a 200.0-mL solution containing 0.050 M benzoic acid (C6H5COOH) and 0.025 M…
A: pH = pKa + log[C6H5COO-]/[C6H5COOH]
Q: 1) Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH;COONa, in 64.0…
A: Answer:- This question is answered by using the simple concept of calculation of pH of solution…
Q: 1) Calculate the pH of a solution prepared by dissolving 2.20 g of sodium acetate, CH3COON,, in 99.0…
A: Here, gievn buffer solutionMass of sodium acetate=2.20gMolarity of acetic acid =0.10MVolume of…
Q: A solution is made by dissolving 26.5 g of LIC3H5O2 in 500.0 mL of water. Using Kb(C3H5O2) = 7.7 x…
A: Given: The mass of LiC3H5O2 = 26.5 g The volume of the solution = 500.0 mL The Kb of C3H5O2- = 7.7 ×…
Q: Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What…
A:
Q: Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine…
A:
Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,1? (Kb of CH,NH, is 4.4 x…
A:
Q: 250 mL pure water at 25C is added with 0.105x10-6 L H2SO4 Solution which contains 98.0 wt % sulfuric…
A: given : Density = mass / volume mass = density × volume = 1.84 × 250 mL mass = 460 g…
Q: 1) Calculate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH3COONA, in 85.0…
A: weak acid and salt of weak acid's combination solution's pH can be predicted by Henderson hesselbech…
Q: What is the pH of a solution prepared by mixing 50.00mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl?…
A: Given data is as follows:
Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…
A:
Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M…
A: Since the moles of acetic acid = molarity of acetic acid X volume in L = 0.1 X 30/1000 = 0.003 And…
Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?
A: Given data, The pOH of a weak base is calculated as shown below.
Q: The PH of a solution of HCL in water is found to be 1.20.What volume of water would be added to…
A: Formula used M1V1= M2V2
Q: 2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium…
A: Given, [CH3COOH] = 0.50 M Volume of CH3COOH = 25 mL [CH3COONa] = 0.30 M Volume of CH3COONa = 25…
Q: Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What…
A:
Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 mL of 0.10 M…
A: Weak acid are those which does not dissociate completely in aqueous solution. Here all CH3COOH are…
Q: What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka =…
A: Given system is buffer mixture
Q: 4) Calculate the pH of a solution that is composed of 90.0 mL of 0.345 M sodium hydroxide, NaOH, and…
A:
Q: Calculate the pH and pOH of the mixture of 10.0 mL 0.0345 M HCl and 10.0 mL 0.000890 M Sr(OH)2.
A:
Q: What is the pH of a solution prepared by adding 2.37mL of 1.78 M HCL to 0.664L of .399 M weak base,…
A:
Q: Bider the litrahion of 100.6 ml of 0.200 M acetic acid (K, = 1.8 x 10) by 0.100 M KOH. Calculate the…
A:
Q: how you determine the pH when 15 ml of 0.100 M HCI is ado 080 M NH3 (K, = 1.6 x 10-6)
A: Given, Kb = 1.6×10-6 pKb = -log(Kb) = -log(1.6×10-6) = 5.82 Molarity of HCl = 0.100 M Volume of HCl…
Q: Consider a solution formed by mixing 50.0 mL of 0.100 M H2SO4, 30.0 mL of 0.100 M HOCl, 25.0 mL of…
A: First step is to find out total volume Total volume = 50 mL + 30 mL + 25 mL + 25 mL + 10 mL = 150…
Q: 1) Calculate the pH of a solution prepared by dissolving 1.00 g of sodium acetate, CH,COONa, in 57.0…
A: Given that : The mass of salt (sodium acetate) = 1.00 gm The concentration of acid (acetic acid) =…
Q: 13 For an aqueous solution of hydrochloric acid with ph= 0.400, what would be the % mass of…
A: Given pH = 0.4 volume = 100 ml = 0.1 L density = 1g/ml
Q: I mix 100 mL of 0.100 M HCl in 250 mL of 0.150 M NH3. I add 50.0 mL of 0.0500 M NaOH. What…
A:
Q: The Ka of hypobromous acid, HOBr, is 2.6 x 10-9. Calculate the pH of a solu tion which is composed…
A: PH of acidic buffer can be calculated as follows
Q: 100 ml of 1 M CH3CO2H solution and add 4 g of NaOH. Calculate the pH of the solution?
A: Given data:
Q: 1) Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH3COONa, in 64.0…
A: Given; The given mass of CH3COONa, (W) = 1.6 g. The molar mass of CH3COONa, (M) = 82.0343 g/mol.…
Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH3CO2H with. 30.00 mL of 0.030M…
A:
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- Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.What weight of potassium hydrogen phthalate will require 30. mL of a 0.30M NaOH solution to reach the equivalence point? KHP MM 204.22 g/mol .CO;K' .CO;K' NaOH + H2O + *CO,H COƠ,Na'5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
- A titration of 29.2 mL of a solution of the weak base aniline, C@HNH, ( K 4.0 x 10-10), requires 21.61 mL of 0.155 M HCl to reach the equivalence point. CH_NHz(aq) + HyO* (aq) + C,H,NH, (aq)+H,O(l) a What was the concentration of aniline in the original solution? Concentration 0115 ✔ M The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus, [C,HNH] [H₂O+] [OH-]- = 0.155 mol HC1 1.00 L 1 29.2 mL b What are the concentrations of H₂O¹, OH, and C6H5NHs at the equivalence point? M C = 0.115 M x 21.61 ml x M Correct 1 mol C, H, NH, 1 mol HCl Show Hint1: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)A 0.2386-g sample contained only NaCl and KBr was dissolved in water and required 50.00 mL of 0.04500 M AgNO3 for complete titration of both halides. If we assume there is x mol of NaCl in the original sample, which of the following statements are CORRECT? There are multiple correct answers. MW(NaCl) = 58.44 g/mol. MW(KBr) = 119.002 g/mol. There is x mol of KBr in the original sample. x+(0.2386-58.44x)/119.002-50.00*0.04500 There is (0.002250 - x) mol of KBr in the original sample. 58.44x+119.002(0.002250-x)=0.2386(f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)Consider an analyte solution of 50.0mL of 0.050M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH (the titration you will be performing in the lab!). (g) After adding 37.50mL of the NaOH, 50% past the equivalence point, what ions or molecules are present in the solution? (h) Which of the species you identified in part (g) will determine the pH of the solution?A butanoic acid/potassium butanoate (C,H,COOH/KOOCC,H,) buffer is prepared to 1.12x10-2 mol L1CH,COOH and 8.38x10-3 mol L1 KOocC;H. The K, for butanoic acid is 1.5x10-5. What is the pH of the buffer solution? Part A O 4.82 O 4.70 O 5.25 O 4.65 O 4.95 o o o o oFill in only the appropriate boxes in the ICE table below as you would to answer the following question: What is the concentration of H30* in a 0.2 M solution of HCIO3 in water? (Only fill in the ICE table; actual calculation of [H3O+] is not required). H20(1) HCIO,(aq) I | C CIO;"(aq) E HCIO,H*(aq) H;O*(aq) || OH"(aq) 0.2 0.2-x | 0.2+x -X +X X | Please put an answer in each box. 11The hydroxide ion concentration of an aqueous solution of 0.490 M acetylsalicylic acid (aspirin), HC,H;04. is [OH] = |M.SEE MORE QUESTIONS