2- A CO3 free NaOH solution was found to be 0.0712M immediately after preparation. If exactly 2.0L of this solution was exposed to air for some time and absorbed 0.416g Co..Calculate the carbonate concentration in solution(M.wt=44.0g /mol)? Select one: 0.76M 0.037M 1.36M 0.0047M
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- 25.0 cm³ sodium hydroxide is neutralized by 15.0 cm³ sulphuric acid of concentration 0.10 mol dm-3. a. Write the equation for the reaction b. From the equation, determine how many moles of sulphuric acid will neutralize 1.0 mol of sodium hydroxide. c. Determine how many moles of sulphuric acid are used in the neutralization. d. Determine the concentration of sodium hydroxide.5. The concentration of H₂SO3 in a saturated aqueous solution at room temperature is approximately 0.10 M. Calculate [H3O*], [HSO3], and [SO32-] in the solution: Ka1 1.0 x 10-2, Ka2 = 6.0 x 10-8 1 C e + H₂SO₂H₂O + HSO₂" HS03 0.10 M 0.10M-X O +X X 2 (H₂0°) (HSO₂) _x² (H₂SO₂) (0.10-x) Val =1₁0×10²² = x ² (0.10) 0.40 10.01=1x² 0.032= X Assume x <<<0110-x 0.10- 20.10 (040) Validity = 0.032x100, 0.10 = 0.32% <5%Q1) A sada- Lime Sample is 90% NaoH and 10% CaO• If 3gm is dissolved in 250 ml, what is the tutal normadity of the Selution as abase ? How many milliliters of O.57N H2 S@4 would be requiredd to titrate i00 me of the Solution ? Ans.s ( 0.309 N, 60.59 ml) Q12) How much water that required add to 200 ml HNO, ( densly = 1.285 gm/ml) Contains 46 wt% acid to Convert lo wt% acid solution? Ars. : 919.6 ml
- A 2.1562 g sample that may contain NaOH, NaHCO3 and Na2CO3 alone or in compatible mixtures reqıires 31.2 ml of 0.1082 M HCl for titration to the phenolphthalein end point and additional 52.4 ml of the same acid to bromocresol green end point. Calculate the percentages of compound(s) in the sample (M. Mass of NaOH:40 g/mol, M. Mass of NaHCO3: 84.01 g/mol, M. Mass of Na2CO3: 105.99 g/mol)?Answ GA 20. Answ My C X C Write C The F X C Whe x akeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. When 25.0 mL of a 1.99×104 M lead nitrate solution is combined with 15.0 mL of a 6.28×10-4 M sodium iodide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to Submit Answer Retry Entire Group 1 more group attempt remaining क Ni ENG US Home End InsFe3+ undergoes four separate hydrolysis reactions in solution. Log Kh for each reaction is as follows: log Kh1 = -5; log Kh2 = -10; log Kh3 = -15; log Kh4 =-20. Which species of Fe would be most prevalent in water with a pH between 5.5-7?
- Pbl2 in H2O has a KSP equaled to 8.0 x 10^-9. If there is 1L of H2O, how many moles of Pbl2 can be dissolved?.24. Methylamine, CH3NH4 is a weak base that ionizes in solution as shown by the following equation. CH3NH2 + H20 5 CH;NH;* + OH- (a) At 25 °C, the percentage ionization in a 0.160 molar solution of CH3NH2 is 4.7%. Calculate JOH], [CH3NH3'], [CH3NH2], [H3O*], and the pH of a 0.160-molar solution of CH3NH2 at 25 °C.made upetement Zazum Adomica Abmcmas rop 418.28 Specific heat 19.42 173 13
- 1.What is the molarity of a solution made from placing 0.2200 g tartrazine powder in a 1L volumetric flaskand diluting it to the mark? Hint: the solution’s total volume is 1.000 L. 2. What is the concentration of a solution that takes 10.00 mL of a stock solution (4.12 × 10-4 M) and diluteit to 100.00 mL.2. Explain why the observed color change with bromcresol green for each of the four solutions is reasonable given the pH. a. NaC.pH=7 b. Na;CO, pH =10.8 c. NaC;H,O, .pH-8.9 d. NaHSO.pH-1.5 Part C: 1. What was the unknown weak acid? From your observed pH calculate the [H+] concentration in M(mols/L) for your unknown acid 2. Calculate the Ka for the unknown acidDissolve 5.0 g aluminium in 150 cm3 of 25 m/m % (with density of 1.06 g/ cm3) sulfuric acidsolution. What is the mass of the produced Al2(SO4)3 ?MM[Al]=26.98 g/molMM[H2SO4]=98.08 g/molMM[Al2(SO4)3]=342.2 g/mol