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# Titration of a ml solution of hydrochloric acid requires ml of m sodium hydroxide what is the

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e of a weak acid in 32.9 mL of water is titrated with 0.0755 M Ca(OH)2. Calculate the molarity of the weak acid being utilized in the titration above. (do not provide units and follow significant figure rules).
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a solution of hydrochloric acid (HCl). The molarity of the HCl is unknown molarity. If 0.0250 L of the standard solution is used and this reacts with 25.00 mL of HCl, what is the molarity (mol L-1) of the HCl?
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at is the molarity of the hydrochloric acid solution? (HINT: Write and balance the equation first!)
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tion. What is the molarity of the calcium hydroxide solution? (Write and balance the equation first!)
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titrated with a 0.200 M solution of the base, LiOH. Write the balanced chemical reaction for neutralization reaction: HClO4 (aq) + LiOH (aq) → LiClO4 (aq) + H2O (l) Write the NET ionic equation for the neutralization reaction. OH⁻ (aq) + H⁺ (aq) → H2O (l) Compute the pH of the titration solution. Show your work i) before any of the base is added ii) after 25. mL of base is added iii) after 50. mL of base is added A student performs the titration with the same chemicals but with smaller volumes of each chemical . Which of the following titration curves could represent the titration. Explain A because this entails a strong acid and a strong base. Question 2 A student performs a titration of an unknown acid with a strong base and gets the following titration curve: a) The student consults the list of pKa of acids shown below. If the acid is listed in the table below, which is the most likely identity of the unknown acid? Explain. Acid Ka HF 7.2 x 10-4 CH3COOH 1.8 x 10-5 H2CO3 4.3 x 10-7 HBrO 2.0 x 10-9 The unknown acid is HBrO because the calculated Ka is in between 50^-4 and 50^-6 and 2.0 x 10^-9 lies in between them. b) What is the initial molarity of the acid? 10^-3 = 0.001M Question 3 a) Describe the components and the composition of an effective buffer solution. Explain how the components of the buffer allow the buffer to maintain its pH. An effective buffer solution has a weak acid and its conjugate base or a weak base and its conjugate acid. A buffer solution is most effective when the ratio of its component concentrations is close to 1, also when the pH is equal to the pka of the acid.; The components of the buffer allow the buffer to maintain its pH because buffers can absorb excess H+ions or OH– ions. An employer is interviewing four applicants for a job as a laboratory technician and asks each how to prepare a buffer solution with a pH of 5.0. The following constants may be helpful: hydrazoic acid, pKa = 4.74 Boric acid, pKa = 9.23 Archita A. says she would mix equal molar solutions of hydrazoic (HN3) and sodium azide (NaN3) solutions. Bradley B. says she would mix equimolar Boric acid (H3BO3) and HCl solutions. Carlos C. says he would mix equimolar Boric Acid (H3BO3) and sodium dihydrogen borate (NaH2BO3) solutions. Delia D. says he would mix equimolar hydrazoic Acid (HN3) and NaOH solutions. b) Which of these applicants has given an appropriate procedure? Explain your answer Delia because she is using Sodium hydroxide which results in a pH of 5. NaOH is a strong base and in order to have an effective buffer a weak acid must be incorporated which is the HN3. c) Explain what is wrong with the erroneous procedures. The rest all incorporate a strong acid and a strong base or a weak acid and a weak base which don’ result in an effective buffer. d) The applicants have access to the 1 Liter volumes of each of the solutions listed above. They have access to graduated cylinders. In order to make 1.0 Liter of the correct 5.0 buffer solution, what volumes of the two chemicals must be mixed?
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lar mass -KMnO4 = 158 g/mol) used in titration of 100 mL raw-water sample diluted 1:20 was 9,2 mL. Calculate the orientative amount of Fe(III)-sulfate coagulant needed to be added to 600mL of water sample in a coagulation-flocculation experiment.
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ric acid. Titration of 11.3 mL X with 0.119 M silver nitrate required 78.2 mL of the latter. The resulting precipitate, containing a mixture of Ag2CrO4 and AgCl, was dried and found to weigh 1.420 g. How much 0.142 M sodium hydroxide should be used to neutralize 11.3 mL solution X?
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acid. Titration of 13.6 mL X with 0.139 M silver nitrate required 40.7 mL of the latter. The resulting precipitate, containing a mixture of AgBr and AgI, was dried and found to weigh 1.260 g. How much 0.117 M sodium hydroxide should be used to neutralize 13.6 mL solution X?
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1.AU MAT 120 Systems of Linear Equations and Inequalities Discussion

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