Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is 1.8 x 10-5
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Q: The pH of a 1 M NaHCO, solution is 10.5. What is dominant at this pH, benzoic acid (the conjugate…
A: Weak acid is that which does not dissociates completely in aqueous solution, rather maintain…
Q: At 25°C, calculate the pH of a 0.426 M solution of the salt KNO2. (Ka (HNO2) = 4.50 × 10−4 ).
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Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…
A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…
Q: CH3NH2 is a weak base (?b=5.0×10^−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…
A: CH3NH3NO3 → NO3- + CH3NH3+ Kb for the above reaction is 5x10-4 CH3NH3 can donate a proton and…
Q: Enter your answer in the provided box. Calculate the pH at 25°C of a 0.25 M aqueous solution of…
A: Given data:
Q: What is the pH of a 0.220 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
A: Aniline is a weak base. C6H5NH2+H2O⇔C6H5NH3++OH- 1 0…
Q: Calculate the pH of each of the following solutions at 25°C. a 0.125 M HONH2 (K = 1.1 x 10-8) %3D pH…
A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is
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Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution? Kb for triethylamine is…
A: Given, 0.350 M triethylamine Kb for triethylamine is 5.3 *10-4
Q: If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?
A: From the relation, pOH is calculated as,
Q: The benzoate ion, C6H5COO-, is a weak base withKb = 1.6 x 10-10. How many moles of sodium benzoate…
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Q: Which of the following is the pH of the solution containing 0.01 mol CH3COOH and 0.820 grams of…
A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…
Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.54. What is the Kb of this base?
A: pH = -log[H3O+] Where [H3O+] is the concentration of hydronium ion…
Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M solution of methylamine?
A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…
Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…
A: Go through the image provided
Q: What is the pH of a 0.290 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
A: Find PH using ICE table and some farmula
Q: What is the pH of a solution made from combining 2.49 mol (CH3)2NH2Cl and 5.18 mol (CH3)2NH in a…
A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…
Q: Calculate the pH of the following solutions at 298K: (a) potassium hydroxide 2.4 x 104 mol dm3 (b)…
A: To calculate the pH of the below given solution: molarity of KOH = 2.4×10-4 mol dm-3 molarity of…
Q: Calculate the pH of an aqueous solution at 25°C that is 0.28 M in phenol (C&H5OH ). (K, for phenol…
A:
Q: Calculate the pH of an aqueous solution at 25°C that is 0.29M in phenol (C,H;OH ). (K, for phenol =…
A:
Q: how do you counstruct a pH curve for a triprotic acid? For example 75.00 mL of 0.137 M H3PO4 with…
A: The acid dissociation constants for phosphoric acid are quite different from each other with pKa's…
Q: The pOH of an aqueous solution of 0.590 M quinoline (a weak base with the formula C9H7N) is…
A:
Q: What is the pH of a 0.85 M H2SO4? Show your ICE table and calculations. Ka1 for H2SO4 is a very…
A: The sulfuric acid completely disassociates in the solution, hence we can assert that the…
Q: A solution is prepared at 25 °C that is initially 0.37 M in nitrous acid (HNO,), a weak acid with K,…
A: Since the pH of monoprotic acid buffer is given by Henderson-Hasselbalch equation as where pKa =…
Q: what is the ph of 0.010 M solution of acetic acid? for the acetic acid is 1.8x10-5
A: Given information: Concentration of acetic acid is 0.010 M Ka for acetic acid is 1.8 x 10-5
Q: Calculate the ph of 0.350 M acetic acid whose ionization constant is Ka= 1.8x10-5
A: Given :- concentration of acetic acid solution = 0.350 M Ka = 1.8 × 10-5 To be calculated :- pH…
Q: 1. Determine the pH of 0.055 Moxalie acid (HCO, K.-50x 10 and K-54x 10) Note both steps are…
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…
A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka = 1 ×…
Q: A solution is prepared at 25 °C that is initially 0.44 M in methylamine (CH, NH,), a weak base with…
A: Methylamine is weak base and Methyl ammonium bromide is its salt.so the solution is buffer solution.…
Q: A solution is prepared at 25 °C that is initially 0.14 M in chlorous acid (HC10,), a weak acid with…
A: Buffers are solutions prepared using a weak acid or base together with its conjugate salt (formed…
Q: What is the pH of (3.21x10^-1) M C5H5NHBr?
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: The pH of a 0.46M solution of propanoic acid (HC,H,O,) is measured to be 2.60. Calculate the acid…
A:
Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…
A:
Q: Kb for ammonia (NH3) is 1.76 x 10-5 What is Ka for ammonium, its conjugate acid. (NH4+)
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Q: The Ka for formic acid (HCO2H) is 1.8x10-4, What is the pH of a 0.20M aqueous solution of sodium…
A:
Q: A 0.100 M weak base has a pH of 8.77. What is the Kb value of this base?
A: Given:Let the acid be : MOHpH=8.77also, concentration of weak base= 0.100Mi.e [MOH] =0.100M
Q: 4. Calculate the pH of a 0.012 M benzoic acid, HC;H5O2, solution. Hint: benzoic acid is a mono-…
A: Given data: Benzoic acid = .012M ka(benzoic acid) = 6.5 * 10-5 Hint: benzoic acid is a monoprotic…
Q: NH3 is a weak base (K, = 1.8 x 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a…
A:
Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…
A: Solution -
Q: What is the ph of a 0.70M solution of methylamine? Kb is 4.37x10^-4
A: Since the reaction taking place is ( methylamine = CH3NH2) CH3NH2 (aq) + H2O(l) ----> CH3NH3+…
Q: A solution is prepared at 25 °C that is initially 0.47M in chloroacetic acid (HCH,CICO,), a weak…
A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…
Q: What is the pH of a solution that is 0.071 M LiCN at 25°C?
A: A solution is made up of 0.071 M LiCN at 25 ◦ C. Here, we have to calculate the pH of the solution.…
Q: Acidic / Basic / Solution [H3O*] [OH] pH pOH Neutral? 0.010M HNO3 6.45 x 106 M NaOH "C" 10
A: Since you have asked a question with multiple sub-parts, we will solve first three sub-parts for…
Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…
A: For first ionization : pH = 0.5pKa1 - 0.5logC ..(1) Here, pKa1 = -logKa1 = -log(8*10^-5) = 4.097 C…
Q: What is the pH of a solution made from combining 6.56 mol C6H5NH3Cl and 7.58 mol C6H5NH2 in a 4.37 L…
A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…
Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M solution of…
A: Given : Concentration of (CH3)2NH = 0.103 M And Kb of (CH3)2NH = 5.90 X 10-4 Since (CH3)2NH is a…
Q: Calculate the pH of an aqueous solution at 25°C that is (a) 0.081 M in HI, (b) 8.2 × 10-6 M in HNO3…
A:
Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…
A:
Q: A solution is prepared at 25°C that is initially 0.41M in benzoic acid HC6H5CO2, a weak acid with…
A: The solution is as follows :
Q: What is the pH of a solution containing 0.055 mol L-1 HCOOH and 0.141 mol L-1 HCOO- ?
A:
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- What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.Calculate the pH of a solution prepared by mixing 49.0 mL of butyric acid, HC4H7O2, with 6.15 g of KOH in water. The following data about butyric acid may be helpful: density=0.9595g/mL;K a =1.54105
- The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
- Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.Estimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow. (See Fig. 14-8.)Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?
- What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.Amino 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?
