Q: a
A: SnCl2 is Lewis acid, when this Lewis acid dissolved in water then this salt will release H+ ion it's…
Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?
A:
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A: Strong acid is fully dissociated in solution
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A:
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A: The given equilibrium reaction is as follows, H2NNH2(aq) + H2O(l) ↔H2NNH3+(aq) + OH-(aq) The…
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A: Given :- concentration of HI solution = 1.02 M To calculate :- pH of the solution pH = -log[H+]
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A: Given: 0.62M NH4NO3
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A: Answer:- This question is answered by using the simple concept calculation of Ka value using the…
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A: The pH of the given solutions are as given below:
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A: According to Bronsted Lowry Theory , any molecule that donate H+ atom is an acid and any molecule…
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A: given that concentration of H2 SO4 = 0.025 Ka2 = 1.2 *10 -2 HSO-4→ SO2-4 + H+ 0.025 0 0.025…
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A: pOH is defined as the negative logarithm to the base 10 of OH- ion Concentration pOH = -log10[OH-]…
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Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56
A: The concept used here is based on the acid dissociation constant of an acid which is used for…
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Q: Determine the hydroxide ion concentration in an aqueous solution of HBr with pH = 3.98 at 25 °C.…
A: Given: pH= 3.98 As we know, pH= -log[H+] So, [H+]= 10-pH [H+]= 10-3.98 [H+]= 1.04 ×10-4M…
Q: Determine [OH−], pH, and pOH of a 0.25 MM ammonia solution. For NH3, Kb=1.76×10−5.
A: The question is based on the concept of equilibrium. ammonia is a weak base. so, partially…
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A: Given that, The concentration of the solution in HCl = 0.052 M And the concentration of the…
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A:
Q: 2. Calculate the (OH) and pOH of 0.0750 M NH3. Ka NH,* = 5.70 x 100
A: 2. Given that : The concentration of NH3 = 0.0750 M The Ka for NH4+ is 5.70 x 10-10. We have to…
Q: 3. How is K, obtained by the half-neutralization method?
A: Since you have posted multiple questions, we will solve the first question. Please post rest of the…
Q: Calculate [H3O+] and pH for a 0.317 M solution of HF; Ka = 6.8 × 10−4.
A: Given, Concentration of HF (C) = 0.317 M Dissociation constant of HF , Ka = 6.8×10-4 [H3O+] = ? pH =…
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A:
Q: What is the pH of a solution with a fluoride concentration of 0.20 M ? The Kb for F– is 1.47×10-11 .
A: In order to find the pH of the solution we first write down the given data: Fluoride concentration=…
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Q: What is the pH of a solution with a fluoride concentration of 0.11 M ? The Kb for F– is 1.47×10-11 .
A: The reaction is as follows, The ICE table for above reaction is shown below,
Q: 2. Calculate the pH of a 0.200 M solution of H2SO4. Ka2 for H2SO4 is 1.2 x 102. (Since Kaz is high,…
A: Step -1 we know that PH = -log(H+) H2SO4 - gives two H+ ions in dissociation condition. So, 2 x…
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Q: 12. A 8.5 L sample of a 0.28 M HNO3 solution is mixed with 1.6 L of a 0.64 M HC1 solution. What is…
A: A multiple choice question based on pH calculation, which is to be accomplished.
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Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 × 10-5) O 4.94 O 12.03 O 1 1.05 O 8.02 O 2.09
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Q: Calculate the pH and pOH of the: 0.125M potassium hydroxide (KOH) solution
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Q: Calculate the pH of a solution that is 0.0400 M in a) NaH,PO. b) NaHC:O. c) NaHS
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Q: Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D) 0.100…
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Q: 10. Nitrous acid (HNO2) is a weak acid with a Ka = 4.0 x 104. If 112 mL of a 0.100 M KOH solution…
A: Answer: In this question we have to find out the pH of a buffer solution made of nitrous acid and…
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A: NaClO is a salt of weak acid HClO. It has pH greater than 7 as it is base.
Q: Calculate the pH of the solution produced when 20.0 mL of o.125 mL of each of the following: a.…
A: d) moles of HCl = 0.125×0.02 = 0.0025 mol Moles of HClO4 = 0.2 × 0.5 = 0.01mol Total moles of H+ =…
Q: 165 Determine the pH of (a) a 0.40 M CH,COOH solu- tion, (b) a solution that is 0.40 M CH,COOH and…
A: CH3COOH is a weak acid. To calculate the pH, degree of dissociation is calculated first (α) using…
Q: Calculate the theoretical pH of the solution please 0.100 M aluminum nitrate Hydrated aluminum ion…
A: Al^3+ solution is slightly acidic in nature. This is because Al^3+ has very high ionic potential.…
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- 1) LiF has a pKsp of 2.77. HF has a pKa of 3.17. LiF is dissolved at 0.250 F after addition of strong acid. What is the pH of the 0.250 F LiF solution? Answer: 1.62 2) For the problem above, how many moles of strong acid are added to form 1.000 L of solution? Answer: ? Please solve the second question, not the first question.Solve correctly please. a 0.25 mol sample of a weak acid with an unknown pka was combined with 10 ml of 3 m koh and the resulting solution was diluted to 1.500 L the measured ph of the solution was 3.85 what is the pka of weak acid Please include formulas used and write answer legibly please. Include all steps aswell. Thankyou. Answer is 4.73PLEASE SHOW ALL WORK FOR BOTH PARTS OF THIS QUESTION >>>> THANK YOU>>> What would the hydroxide ion concentration be if the hydrogen ion concentration was 1 x 10-6 M? and What would the pH of a solution that had a hydroxide ion concentration of 3.2 x 10-8 M be?
- What is the pH of 500ml solution conating 0.125 M fornic acid and 0.140 M sodium formate? Include chemical equation What would the pH be if 1mL of 0.5 HBr was added to solution? pka=3.744To prepare the buffer, a total volume of 600 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 1.5 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 2 decimal places)Solve correctly please. Should correct (Need all parts, gpt/ai wrong answer not allowed). Consider the compound: Fe(OH)2 (aq) What are the IMFs present in this substance? Draw the Lewis dot structure for this compound. What is the pH of a 0.448 M Fe(OH)2 solution?
- How did diluting the buffer affect the pH of the buffer solution itself? ( pls explain it asap!) Thank youThe experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is the solution acidic, basic, or neutral? B. Write the balanced net ionic equilibrium reaction. Identify the acid, base, conjugate acid, and conjugate base. Write the cquilibrium expression Kb for the reaction. C. Look up the theoretical pKafrom the CRC Handbook. Please give me all questions solution fastWhat is the pH at which a buffer composed of NH3 and NH4+ would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values
- A solution is made by dissolving 43.5 g of Ba(NO₂)2 in 500.0 mL of water. (a).As NO₂ is a base, write the basic equilibrium equation that exists in solution. (b).What is the value of Kb for NO₂? The Ka of HNO₂ is 4.5 × 10^-4 (c).Determine the pH of the solution Attempts all parts otherwise i will downvote....please provide handwritten solution ASAP.Cr3+ has pKa = 3.80. Find the pH of 0.010 M Cr(ClO4)3. What fraction of chromium is in the form Cr(H2O)w2+(OH)2+?I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)