PART I. MAKING A SOLUTION OF COPPER NITRATE I. 1. OXIDATION NUMBERS In Part A of the experimental procedure, copper metal is added to concentrated nitric acid. The reaction between copper metal and concentrated nitric acid is an oxidation-reduction reaction that is somewhat complicated. 4 HNO3(aq) + Cu (s) → Cu(NO3)2 (aq) + 2 H₂O (1) + 2 NO₂ (g) Consider the balanced chemical reaction given above. Assign the oxidation numbers to each atom in the equation. Cu: H: O: N: 4 HNO3(aq) 2 2 2 + Cu(s) 2 → Cu(NO3)2 (aq) 2 2 2 + 2 H₂O (1) 2 + 2 NO₂ (g) 2 2

Q: 6. Use Lewis structures to show the electron transfer that enables these ionic compounds to be…

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Q: 4. Indicate with a plus sign (+) any of these processes that require energy, and a negative sign (-)…

A: Some process, energy is required. For some process, energy is released depending upon the particular…

Q: Which of the following would be classified as a nonelectrolyte? NaMnO4 HCI CH3COOH CH3OH Question 5…

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Q: How many total atoms are there in seven dozen molecules of nitric acid, HNO3?

A: Answer to question no. 5 (as mentioned); 1 molecule of nitric acid HNO3 contains 5 atoms ( 1 H, 1N,…

Q: QUESTION 7 Predict the major product for the following reaction. 1. ex ce ss CH31 NH2 2. Ag0, H,0…

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Q: 5. Which of the following equations represents the net ionic equation for the reaction? a. Na*(aq) +…

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Q: 4. Make the following conversions and include an equation for each one: (a) 32 °C to °F (b) -8.6 °F…

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Q: 3. What is the concentration (molarity) of a solution made from 12.5 g of calcium fluoride and 250mL…

A: Molarity = number of moles of solute/volume of solution (in L) Number of moles = mass/molar mass…

Q: 13. Which of the following structures contains a secondary amine? NH2 `NH `NH2 II II IV А) I B) II…

A: To Solve this problem first we have to know about primary, secondary and tertiary amines .

Q: Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction…

A: When reaction quotient (Q) is less than equilibrium constant (K) , equilibrium of the reaction moves…

Q: What are the answers to prelab  questions 1-4

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Q: A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)¸N) ³ N) solution with 0.8123 M HCl…

A: Concentration of trimethylamine = 0.2187 MVolume of trimethylamine = 110.0 mLpKb of triethylamine =…

Q: Q2. What do you notice when you compare the initial boiling temperatures for the two concentrations?

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A: Since you have posted multiple questions with multiple sub-parts, we are entitled to answer the…

Q: 1. Give the structures of the products obtained when the following are heated. Ph Me OMe b. a. O,N…

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A: “Since there are multiple questions and it is not mentioned that which one has to be solved so I am…

Q: Arrange the values according to magnitude. Greatest     Least Answer Bank 7.1×10−6 3.3×10−2 52000…

A: 7.1 * 10-6 = 0.0000071, 3.3 * 10-2 = 0.033, 52000,  9.0 * 10-6 = 0.0000090,  2.2 * 105 = 220000

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Q: Answer all questions from

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Q: 5. Which of the following statements about valence electrons is true? A) They are the most tightly…

A: It's a multiple question type.   The above mentioned questions are explained below:

Q: QUESTION 3: Show your solutions for all questions below: 3a. Which mass is greater? 34.0 g of…

A:

Q: Answer 8F

A: The objective of the question is to identify a suitable indicator.

Q: 9. The following compounds are named incorrectly. Draw the structure of each compound and give it a…

A: We have to draw the structures of the compounds and determine the correct name of the compounds

Q: Boxes 1-6 Answer choices: HCHO2, NH4Cl, NH3, NaCHO2•H2O, HC2H3O2, NH4^+, NaC2H3O2•3H2O, C2H3O2^-,…

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Q: I Figue 1-1 4 P sp² 777 工 NEC, 工 Ⓡ •C 3 sp千千千千 H 2 TIC 吓人 以下 p44 sp44 C 3 E H IV 又 不让我下

A: Number of valence electrons of C = 4Number of valence electrons of N = 5Number of valence electrons…

Q: H H H-C-O HHH HHH HHH HHHHH H-C-o HH HHH HH CH, H H 0/2 CH, H H -C-H HH 1. What do you call the…

A: amphipathic molecule that has both polar and non-polar parts.

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.