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Explain why different results are observed when HCl and H2SO4 are added to brine?
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- Explain the role of phenolphthalein in the standardization of NaOH with KHPwhat is the atomic number for Ph, and why does CH2Br have 2 priority over Ph and CH3?(a) Find the pH of a 1.00 L solution prepared with 12.43 g of base (CH2OH)3CNH2 (MW =121.135 g/mol) plus 4.67 g of its conjugate acid (CH2OH)3CNH3Cl (MW = 157.596 g/mol).(b) How many mL of 0.500 M NaOH should be added to 10.0 g of (CH2OH)3CNH3Cl to give a pH of 7.60in a final volume of 250 mLConsider the pKa of (CH2OH)3CNH3+ = 8.072
- Using the letters on the image, identify each component of the titration set-up. Buret clamped to a ring stand with a beaker underneath. The letter A appears at the top of the buret, the letter B appears midway down the buret, the letter C appears at the bottom of the buret, the letter D appears next to the beaker, and the letter E appears on the other side of the buret, near the ring stand.pls complete and explain how to get Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used.…Write the values of Y and X. H2SO4 CH3CH=CH2 + H2O CH;CH-CH2 H HỌ 2-propanol an alcohol The pKa of a protonated alcohol is about -2.5, and the pKa of an alcohol is about 15. Therefore, as long as the pH of the solution is greater than Y and less than X, more than 50% of 2-propanol will be in its neutral, nonprotonated form. Express your answers using two significant figures separated by a comma. AX中 Y, X = %3|
- (4c-201) Copy the following equation, and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid. HNO3 + H2O → H30* + NO3¬ For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial 14px A v ... In X2 田由田図 EX: ABC Ť {;} > >A) Write the Ksp expression for the sparingly soluble compound lead phosphate, Pb3(PO4)2. Ksp = If either the numerator or denominator is 1, please enter 1. b.) Write the Ksp expression for the sparingly soluble compound silver sulfate, Ag2SO4. Ksp = If either the numerator or denominator is 1, please enter 1.Briefly describe how you could separate the components of a mixture of benzoic acid and Na2SO4 and recover the two separated substances.
- MISSED THIS? Read Section 18.6 (Pages 823-826); Watch IWE 18.12. Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. 9.0x10-2 M Cala; K2SO4 Express your answer using two significant figures. [K₂SO4]= ΜΕ ΑΣΦ Submit Request Answer Part C 1.7x103 M AgNO3; RbCl Express your answer using two significant figures. [RbCl] ΜΕ ΑΣΦ Submit Request Answer M MThe K, for acetic acid (CH,COOH) is 1.737 × 10-5. What is the pK, for this acid? pKa = Use the calculated pK, to determine the pH at which [CH,COOH] = [CH,COO¯]. %3D pH =Draw/illustrate the chemical reaction involved in Benedict’s test and explain the purpose of this qualitative test?