QUESTION 5 What is the pH of a buffer system prepared by dissolving 10.70 grams of NH 4CI and 30.00 mL of 12 M NH 3 in enough water to make 1.000 L of solution? K b = 1.80 x 10 for NH 3. 9.26 9.51 O 11.32 9.00 Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save A

Q: Please answer 1,2,3,4 thankyou 1. What effect will addition of sodium acetate have on the pH of a…

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Q: Question 9 Listen E 55.0 mL of 0.30 M HF (K₁ = 7.2 x 10-4)is titrated with 5.0 mL of 0.40 M NaOH.…

A: The reaction between HF and NaOH will be, HF + NaOH -----> NaF + H2O And is given that, 55 ml of…

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Q: Calculate the pH when 32.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH,NH, (Kb = 4.4 ×…

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Q: What mass of ammonium chloride should be added to 2.55 L of a 0.145 M NH3 to obtain a buffer with a…

A: As we know, pKb=-logKb and, pOH=pKb + logSalt[Base]

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Q: QUESTION 11 If the pKa of HCHO2 is 3.74 and the pH of an HCHO2 /NaCHO2 buffer solution is 3.74,…

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Q: Titrating a Strong Base with a Strong Acid Exercise 3: Assume that all solution is diluted with pure…

A: Answer -

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.…

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A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: QUESTION 1 Consider the titration of 20.00 mL of 0.150 M NH3 with 0.250 M HCI. Determine the pH of…

A: NH3 is a weak base which gets neutralized by HCl to give salt (NH4Cl) and water. So, if there is a…

Q: Question 4 A buffer solution includes a weak acid and its conjugate base. Include states of matter.…

A: A buffer is a solution of weak base and its salt. Here, Weak base is NH3 i.e, NH4OH. Salt of weak…

Q: QUESTION 6 A titration of 45.0 mL of 0.17M HNO2 with a 0.25M LIOH solution. What is the pH of the…

A: Given molarity of HNO3 = 0.17 M Volume = 45 mL = 0.045 L So,  Number of moles of strong acid HNO3 =…

Q: 4:32 NaOH? pH A) HF C) OH- Question 13 of 13 B) HF and OH- D) F- A mL OH- Periodic Table Submit D

A: Titration is a laboratory technique used to determine the concentration of a substance in a sample.…

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Q: Macmillan Learning A 50.0 mL solution of 0.172 M KOH is titrated with 0.344 M HCl. Calculate the pH…

A: Note: Since you have posted a question with multiple sub parts, we will provide the solution only to…

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A: pH can be calculated using the following equation: pH = - log (H+) pH of the solution is 3.65…

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Q: Y Part A What relative masses of dimethyl amine and dimethyl ammonium chloride do you need to…

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A: we have to calculate the pH of solution

Q: A solution is made by dissolving 33.5 g of Ba(NO₂)2 in 500.0 mL of water. Using Kb(NO₂) = 2.2 ×…

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Q: Question 17 You titrate a 0.125 L of 0.250 M ammonia solution with 0.500 M HCI. What is the pH at…

A: we have to calculate the pH of solution at equivalence point

Q: Question 5, Listen Consider the following buffer system: 1.15 M H3PO4 and 1.14 M H₂PO4-. What is the…

A: Note: As per the Guidelines solution of 1st question has been made. For the expert solution of 2nd…

Q: QUESTION 4 Over what range of pH is a HOCI/NaOCI buffer effective? O pH 1.0 - pH14.0 o pH 6.5 - pH…

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Q: solution initial components A B с D H₂O H₂O H₂O, NaOH H₂O, NaOH initial type (check all that apply)…

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Q: QUESTION 3 A solution is prepared by adding 100 mL of0.2 M hydrochloric acid to 100 mL of 0.4 M…

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Q: You are making 100mL of a 0.66M phosphoric acid buffer with a pH of 7.0. What is the concentration…

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A: Given data Kb of nicotine (C10H14N2) =1.00×106 pH of the buffer solution = 9.2

Q: 2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NAOH, what is the initial concentration…

A: Answer: 2 Given: Volume of H2SO4 = 358mLConcentration  of  H2SO4 =?? Volume of NaOH=…

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Q: Question 4 I'm not sure how to do this question.

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.