If the pKa of HCHO 2 is 5.74 and the pH of an HCHO 2/NaCHO 2 solution is 6.11, which of the following is TRUE? a [HCHO2] >> [NaCHO2] b [HCHO2] > [NaCHO2] c [HCHO2] < [NaCHO2] d [HCHO2] = [NaCHO2]
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a |
[HCHO2] >> [NaCHO2]
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b |
[HCHO2] > [NaCHO2]
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c |
[HCHO2] < [NaCHO2]
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d |
[HCHO2] = [NaCHO2]
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- Each row represents an experimental “run” (in this case, averaged sample of mango wine). Column A shows the run number; Column B shows the percentage of ethanol; Column C shows the amount of glycerol (in g/L); Column D shows the amount of acid (in g/L); Column E shows the temperature of the run (in °C); and Column F shows the pH of the run. Y represents Ethanol of mango wine. 1. Create a scatterplot of the ethanol data for all 20 runs a. Draw a graphical representation of the model that you chose to use. b. Comparing the model to your data, evaluate its fit in one or two sentences. (Not sure what this question is getting at. I've provided all the information given) c. Replace the generic Yi = β0 + ε with the information you have here. Please help. I have no idea what this even means or where to start. HERE is the attached dataset to start with; a b c d e f Run Ethanol Glycerol Acidity Temp pH 1 4.8 3.5 0.84 24 3.8 2 9.6…The pKa of acetic acid, HC2H3O2 is 4.58. A buffer solution was made using an unspecified amount of acetic acid and 0.4 moles of NaC2H3O2 in enough water to make 1.87 liters of solution. It's pH was measured as 3.11. How many moles of HC2H3O2 were used? Report answer with 2 places past the decimal point.Calculate the pH of a 0.50 L solution when 1.00 ml of 1.5 M formic acid and 2.0 ml of 0.4 M formate are added to it. (pK of formic acid = 3.75)
- Sulfurous acid, H2SO3, is diprotic: pka1= 1.81, pka2= 6.91. Calculate the concentrations of all acid species: [ H2SO3 ], [ HSO3¯ ], [ SO3²- ], the pH and the pOH in a 1.9 mol L-1 solution of Sulfurous acid. [H₂SO3 ] = __ mol L-1, [HSO3¯ ] = __ mol L-1, [ SO3²- ] = __ pH = mol L-1, pOH =1. What is the pH of a solution of 20.0 mL of 2 M KOH with 20mL of 2 M HF? (ka = 7.2e-4 and kb = 1.4e -11) 2. What is the pH of a solution of 20.0mL of 2 M HF with 60 mL of 2 M KOH? (ka = 7.2e-4) and kb = 1.4e -11)Calculate the pH value of a solution consisting of 100 mL of KOH 10^-1 mol/L and 100 mL of CH3COOH 10^2 mol/L. The following pKa is given: pKa(CH3COOH/CH3COO-)= 4.8
- Report your ratio/answer as a decimal. The pKa of acetic acid is 4.75. What is the ratio of the concentration of sodium acetate to the concentration of acetic acid at pH 5.75? [sodium acetate] [acetic acid]=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|What is the pH of a solution containing 0.12 mol/L of NH4Cl and 0.03 mol/L of NaOH (pKa of pKa NH4+/NH3of is 9.25)?
- If the pKa of HF is 3.14 and the pH of an HF/NaF solution is 3.04, then_. [HF]=[F] [HF]>>[F°] O [HF][F] [HF]<[F]I have ammonia (20 M) dissociating in water. What is the pH? (4 sig figs). Kb= 1.8x 10-5A.) What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid, HC3H5O2, Ka = 1.3 x 10-5 at 25°C.) B.) What is the pH of a 0.79 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25oC?