17. Oxygen has 6 electrons in its outermost shell. It generally accepts 2 electrons to complete it's octet. The oxidation state of oxygen is usually -2 except in peroxides (H2O2) where it is -1, and in compounds with fluroine (OF2) where it is +2.
Hence, Option-D i.e, -2 is the correct answer.
18. Acetic acid is a weak acid and sodium acetate is the salt of its conjugate base. Hence, acetic acid and sodium acetate forms a buffer solution whose pH can be calculated by using Henderson hesselbatch equation:
pH = pKa + log([conjugate base]/[weak acid])
=> pH = pKa + log([sodium acetate]/[acetic acid])
=> pH = 4.75 + log(0.20M / 0.35M)
=> pH = 4.5069 or 4.51 (approx)
Hence, Option-C i.e, 4.51 is the correct answer.
19. The reaction is spontaneous if the value gibbs free energy (∆G) is negative. The formula for gibbs free energy is:
∆G = ∆H - T∆S
When ΔH is negative and ΔS is positive, the sign of ΔG will always be negative, and the reaction will be spontaneous at all temperatures
Hence, Option-B i.e, all temperatures is the correct answer.
20. During titration, at complete neutralization,
No of moles of acid = No of moles of base
As, Molarity = no of moles/Volume
=> No of moles = Molarity * Volume
Thus, ( M * V) HCl = ( M * V) NaOH
M(HCl) * 25.87 mL = 0.1146M * 28.16 mL
=> M(HCl) = 0.1247 M
Hence, HCl concentration is 0.1247 M. Option-c is the correct answer.
17. In a compound, oxygen generally has an oxidation number (state) of A) +2 B) +1...
20. 25.87 mL of aqueous HCl is titrated to endpoint with 28.16 mL of aqueous NaOH. The NaOH concentration is 0.1146 M. What is the HCl concentration? A) 0.1146 M B) 0.2292 M C) 0.1247 M D) 0.0624 M 21. 13.5 g of NaCl is dissolved in 100.0 g of H20. The boiling point of the water after the salt is added is The boiling point elevation constant for water: K = 0.512 °C/m. A) 102.4° C B) 101.2°C C)...
1. Determine the number of moles of reagent in the following solutions: a. 25.00 mL of 0.10 M acetic acid b. 5.55 mL of 0.092 M NaOH C. 0.50 mL of 0.087 M HCI 2. A buffer solution contains 0.120 M acetic acid and 0.150 M sodium acetate. a. How many moles of acetic acid and of sodium acetate are present in 50.0 mL of solution? b. If we add 5.55 mL of 0.092 M NaOH to the solution in...
1. A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of this solution after 5.00 mL 10.0 M HCl is added? 2. Which of the following solution(s) is a buffer? 100 mL of 0.1 M acetic acid mixed with 25 mL of 0.5 M NaOH 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.05 M sodium...
(2) Find the oxidation numbers of the bold-labelled atoms in the following species: (a) CrF4 (b) UO3 (c) HReO4 (d) FeO42- (e) BrO3- (f) PH4+ (3) Suppose you have a 2.30 M solution of rubidium hydroxide and you are asked to make up 500.0 mL of 5.00 x 10-3M rubidium hydroxide. How much of the stock solution do you need? (4) How many grams of sodium formate (NaCHO2) do you need to make 250.0mL of 7.50 x 10-3M solution? (5)...
1. Which of the following make a buffer solution? (circle all the correct answers) a. 0.1 M HCl and 0.1 M NaCl b. 0.1 M HF and 0.075 M KF C. 0.15 M Pentanoic acid and 0.15 M sodium pentanoate d. 0.1 M NaOH and 0.1 M HCI e. 0.1 M acetic acid and 0.00001 sodium acetate 2. Which of the following could make buffer systems when mixed together? (circle the correct answers) a. 0.10 M acetic acid and 0.05...
1- A) How many milliliters of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of acetic acid (CH3COOH), a monoprotic acid? View Available Hint(s) B)What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH solution for neutralization? C))What is the concentration of a phosphoric acid solution of a 25.00 mL sample if the acid requires 42.24 mL of 0.135 M...
i need equations for question 2
a) Dissociation of a strong base in water b) Dissociation of a strong acid in water c) lonization of a weak base in water d) lonization of a weak acid in water e) Autoionization of water 3. A 5.0 M solution of HCl in water has a proton concentration of M. 4. A0.01 M aqueous NaOH sohution has a hydroxide concentration of M 5. An aqueous HCl solution has a proton concentration equal to...
DATA TABLE Buffer A Buffer B Mass of NaC2H3O2 used to prepare buffer (g) 0.149 g 1.49 g Volume of buffer prepared (mL) 100.0 100.0 Molar concentration of HC2H3O2 in buffer (M) 0.1 1.0 Initial pH of buffer 4.24 4.33 Volume of 0.5 M NaOH to raise pH by 2 units (mL) 1.5 19.0 Volume of 0.5 M HCl to lower pH by 2 units (mL) 1.0 5.0 Volume of 0.5 M NaOH at equivalence point (mL) 1.75 19.75 3. ...
Worksheet 2 2. Calculate the concentration of each of the following solutions. Determine the molarity (mol/L) of a solution made by diluting 5.880 g of barium chloride to a final volume of 525.0 mL a. b. What is the molarity of a solution that dilutes 12.50 mL of 6.00 M HCI (hydrochloric acid) to a final volume of 1.50 L? If you combine 1.55 g of NH CI (ammonium chloride) with 2.38 g of CaCl, (calcium chlo- ride) and dilute...
For the buffer we prepared in the procedure, when the buffering
effect fail? (Hint: This is equivalent to asking when will we
exceed the buffer's capacity?)
Procedure I. Obtain a pH meter and calibrate it if necessary ll. Acids comparison a. Prepare 100 milliliters of an aqueous solution of oxalic acid dihydrate at a concentration 0.010 M b. Determine the pH of the resulting solution. c. Repeat parts a and b on the same volume of solution atthe same concentration...