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write the balanced equation for the hydration of cuso indicate the physical states using the abbreviations s l or g


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1.AP Chem AB FRQ Question 1 A sample consisting of 50. mL of 0.400 M solution of the acid, HClO4, is titrated ...

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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2. Write the balanced equation for the hydration of CuSO4. Indicate the physical states using the abbreviations (s), (l), or (g) ...

reviations (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) to indicate the aqueous phase. Indicate appropriate charges on negative and positive ions if they are formed.
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3.Write the balanced molecular equation, complete ionic equation and the net ionic equation for the reaction between an aqueous solution ...

action between an aqueous solution of Ammonium phosphate and the aqueous solution of Chromium (II) nitrate. Make sure to include physical states in all three equations.
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4.. When 4.00-L of 0.0290 M aluminum sulfate and 3.25-L of 0.0700 M Pb(NO3)2 solutions are mixed, solid lead (II) ...

d lead (II) sulfate precipitates (a) Write a balanced chemical equation for the reaction (b) Write the net ionic equation for the reaction (c) What type of reaction is occurring? (d) What is the limiting reagent? The excess reagent? (e) How many grams of lead (II) sulfate are formed? (f) In the lab, a chemistry student mixed the two solutions together and formed 9.40 g of lead (II) sulfate. What percent yield did the student obtain?
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5.I have to write half-reactions for my pre-lab but I've never learned anything like that and don't have a clue ...

ve a clue at how to do it. 1st Take 2mL of the NaHSO3 solution. Add a drop of dilute HCl solution then add .02M KMnO4 solution one drop at a time, mixing after each drop, up to no more than 5 drops. What changes did you see? Test for SO42- by adding .1MBaCl2 solution one drop at a time, mixing after each drop, up to 6 drops. Write the balanced half-reaction equation for the oxidation of the bisulfite ion, HSO3-.
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1.AU MAT 120 Systems of Linear Equations and Inequalities Discussion

mathematicsalgebra Physics