The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKą of the acid 5.74? 0.0576 M OA. 0.387 M O B. 0.657 M OC. OD. 0.274 M 0.315 M OE.
Q: а. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where: H2Stag) > H*(ag) + HS…
A: pH is defined as negative logarithm of hydrogen ion concentration and it is represented as pH =…
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A: Strong acid is fully dissociated in solution
Q: What is the pH of 6.0 x 104 M HF? The K, for hydrofluoric acid is 7.2 x 104. O a. 2.95 b. 3.22 C.…
A: Answer:- This question is answered by using the simple concept of ionisation of weak acid and then…
Q: how many moles of ammonium nitrate would be required to prepare .40 L of solution that is ph 5.40
A: NH3 + HNO3 → NH4NO3 weak base strong acid salt Salt…
Q: 19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate…
A: Given: Mass of NH4NO3=48.026g Molar mass of NH4NO3=80.043 g/mol Volume =2.00L…
Q: The pKa for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.25 O b. 1.24 O c.…
A: this is the salt of weak acid and strong base. so ,we will use hydrolysis equation of weak acid and…
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A:
Q: The pH of a 0.15-M solution of HSO4− is 1.43. Determine Ka for HSO4− from these data.
A: Given, initial concentration of HSO4− = 0.15 M pH = 1.43 We know that, pH is the negative…
Q: Formic acid (HCHO,) has a K, 1.8 x 10. What is fractional composition (a) of formic acid in solution…
A:
Q: What would be the pH of a solution of hypobromous acid (HOBr) prepared by dissolving 9.7 grams of…
A: given: mass of HOBr = 9.7 g molar mass of HOBr = 96.91 g/mo moles of HOBr = 9.796.91= 0.1 moles…
Q: A 0.107 M solution of Providenol, a weak acid, has a measured pH of 4.32. Determine the pKa of…
A: The equilibrium constant depicting dissolution of either weak acids/base is known as dissociation…
Q: A sodium hydroxide solution was prepared by dissolving 7 g NaOH in 1 L solution. What is the pH of…
A: By definition, Molarity=number of moles of solutevolume of solution in L The moles…
Q: What is the pH of a 0.015 M HCIO4 solution? a. 1.82 O b. 12.18 C. 0.015 d. 0.030
A:
Q: For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) H,NNH3+ (ag) + OH (ag) K, is 3.0…
A: The given equilibrium reaction is as follows, H2NNH2(aq) + H2O(l) ↔H2NNH3+(aq) + OH-(aq) The…
Q: Determine the pH of a 0.100 M aqueous solution of NaOcI. Data: pK,[HOCI] = 7.40 А 10.20 B 9.75 C…
A: 1- First we will see the Ka from its pKa : pKa = -log(Ka) -pKa = log(Ka) 10-pKa = Ka Ka =…
Q: 13.2) a) A 0.439-M aqueous solution of a weak acid has a pH of 4.56. Calculate Ka for the acid.…
A: Please find the solution as hand written note.
Q: The pH of an aqueous acid solution is 6.15 at 25 ° C. Calculate the Ka for the acid. The initial…
A: The equilibrium constant for acid dissociation is denoted as Ka. It represents the ratio of the…
Q: 6. _C₂H4(g) + O2 (g)=CO₂ (g) +____ _H₂O (1) - If 10 moles of ethylene reacts with 9 moles O₂ to…
A: Given : 1. Moles of ethylene = 10 moles Moles of O2 = 9 moles Moles of CO2 produced = 2 moles…
Q: I'm not sure how to solve 115. I saw one solution that used the ka to solve it, but I don't…
A: For polyprotic acids, the dissociation of acid occurs into multiple steps but the major dissociation…
Q: Which of the following aqueous solutions has the lowest pH: 0.1 M HCL; 0.1 M acetic acid (pKa=4.86);…
A: Both the acetic acid and formic acid are weak acid . Thus they dissociates very small. Thus…
Q: A sample of fruit juice is found to have à hydrogen concentration of 2.87 x 104. What would the pH…
A: Given hydrogen ion concentration of fruit juice is 2.87*10-4. We have to determine PH of fruit…
Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…
A: Hypochlorous acid, HOCl(aq) is a weak acid with Ka = 2.5*10-8 Hypochlorite, ClO-(aq) is a conjugate…
Q: An aqueous solution of a weak acid, HA is prepared by dissolving 0.030 mol of HA in water to yield…
A:
Q: If the pH of a 0.0850 M solution of HB1O2 is 2.29, then what is the value for the acidity constant,…
A: HBrO2 + H2O → H3O+ + BrO2-Initial 0.0850…
Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…
A:
Q: What is the pH of a 6.3 x 10³ M solution of HCI? [Molar mass of HCl=36.5 grams/mole] a) 6.3 d) 8.00…
A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…
Q: The pk, for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.95 O b. 1.24 O c.…
A:
Q: Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of…
A: A solution formed by the addition of a weak acid to the salt of its conjugate base anion is known as…
Q: Consider an initial 0.040M hypobromous acid (HOB) solution at certain temperature. HOBr H*(0) +…
A:
Q: 5. The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction: HbH*(aq) + 02…
A: This problem can be solved by using the Le chatlier's principle. According to Le chatlier's…
Q: What is the pH of a solution containing 5.5 x 10S M OH? O a. 10.29 O b. 7.00 Oc 9.74 O d. 5.47
A: The hydroxide ion concentration of the given solution is = 5.5×10-5 M The pH of the solution is =?
Q: a. A solution of HNO3 has a pH of 3.69. What is the molarity of the solution? Molarity |M b. A…
A: We know that, HNO3 is strong acid. So, it is completely dissociated. Thus, pH= -log[H+] Thus, [H+]…
Q: The pOH of a solution is 9.60 Calculate the hydrogen ion concentration in this .solution x 10-9 M…
A: given, pOH = 9.60
Q: Four bases are prepared as 0.100 M aqueous solutions, which is the weakest base with the lowest pH?…
A: Kb is dissociation constant. It measures how completely a base disoociates into components ion in…
Q: THe pOH of 0.5 M solution of weak base is 4.72. What is its pKa?
A: Given-> pOH = 4.72 Molarity =0.5 M
Q: Why is rainwater always acidic, even in the absence of polluting gases such as SO3?
A: The rain water is acidic due to the presence of carbon dioxide, sulphur dioxide and nitrogen dioxide…
Q: What is the pH of 500.0 mL of a 0.1 M NaOH solution? O A. 13 О В. 1 ОС. 1.3 O D. 12.7 47L Ansuers to…
A: Given : Concentration of NaOH solution = 0.1 M
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A: Strong acids and strong bases dissociate completely in their aqueous solution to provide H3O+ and…
Q: What mass of HClO4 must be present in 0.500 L of solution to obtain a solution with each pH value?a.…
A: The answer for part (a) is given below. Kindly repost the other parts as separate one.
Q: 16.62
A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…
Q: HC2HO3 (aq) _ H2O (l) H3O+ (aq_ + C2HO3- (aq) pKa =3.18 at 25C The equilibrium for the acid…
A: pH = pKa + log[salt]/[acid] Number of mmol = Molarity × Volume in mL
Q: The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction:HbH+(aq) +…
A: Hemoglobin is the only protein in the human body that helps in the oxygen transportation throughout…
Q: please highlight the correct answer
A:
Q: A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. N: 14, H:1, S:32, O:16…
A: A buffer solution is an aqueous solution consisting of a mixture of weak acid and it's conjugtae…
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A:
Q: In determining the pH of 0.010M solution of weak acid, HCNO, which equations are relevant in the…
A: Ka= 3.47x 10-4
Q: What is the concentration of H+ in moles/L in a solution that has a pH of 8.35?
A: Given :- pH of solution = 8.35 To calculate :- concentration of H+ ion (mol/L)
Q: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…
A: HA + H2O ↔ H3O+ + A- Ka = [H3O+] [A-][HA] It is given that,the concentration of the weak acid…
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A: 1. Conjugate bases are species obtained from acid by removal of proton from an acid. They are…
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- The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/AA buffer solution containing 0.19 M methylammonium and 0.22 M of the conjugate base, methylamine, was prepared. The pka of methylammonium is 10.64. What is the pH of this buffer solution? Oa. 5.68 Оb. 10.64 Oc. 10.70 Od. 3.42 Oe. 10.58Calculate the pH of a solution that is 0.080 Min trimethylamine, (CH3)3N, and 0.13 Min trimethylammonium chloride, ((CH3)3NHCI).
- Acetic acid (pK, = 4.76) was dissolved in an aqueous solution buffered to a pH of 5.76. Determine the ratio of the concentrations of acetate ion and acetic acid in this solution. Which species predominates under these conditions? O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.01. O Neither species predominates, because the ratio of [acetate ion]/[acetic acid] = 1. O The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 10. The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 100. %3D O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.1.An analytical chemist is titrating 247.8 ml. of a 0.6300M solution of nitrous acid (HNO₂) with a 0.9300M solution of NaOH. The pK, of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 118.8 ml. of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH- 0 GThe pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.
- 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?22) Consider the titration of a 50.00 mL sample of 0.200 M benzoic acid with 0.200 M NaOH (aq., 25 °C). The K CH,COOH = 6.30 x 10*. Calculate the pH of the solution after 25.00 mL NAOH has been added. b) 5.47 e) 4.20 c) 6.65 f) 9.42 a) 3.86 d) 8.34In the laboratory, a general chemistry student measured the pH of a 0.433 M aqueous solution of phenol (a weak acid), CoH5OH to be 5.167. Use the information she obtained to determine the K, for this acid. K₂(experiment) =