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Find the fraction in the form NH3 at pH 10.00.
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- A weak base has KB = 3.26 x 10-2. What is the pKB of this base? Report your answer to at least 1 decimal place.a HF, HI, Nal, NaF Increasing pH of 0.10-M solution Drag and drop your selection from the following list to complete the answer: Nal NaF HI HF Ь н,NNH, CI, HCІ, КСІ, Н2NNH, Increasing pH of 0.10-M solution Drag and drop your selection from the following list to complete the answer: KCI H2NNH2 HCI H2NNH3 Cl OGH ΝΗΝ Ο, NaNO, NaOH, HOC, H5, ΚOC, Hs , C5Η5 Ν, ΗΝΟ; K (C; H;N) = 1.7 x 10-9 K. (HOC,H;) = 1.6 × 10-10 Increasing pH of 0.10-M solution Drag and drop your selection from the following list to complete the answer: C; H;NHNO3 NaNO3 NaOH HNO3 C5 H; N KOC,H5 HOC,H5Where Kal = 4.20 x 10-7 Ka24.69 × 10-¹1 X (a) Calculate the fraction H₂CO3, HCO3, CO3², use the following table as your template. (b) Plot_p¹ vs. fraction of H₂CO3, HCO3, CO3² using the plotting guidelines all on same chart. pH [H] “H_co, ан,со, анс, а со α α 1.806 2.020 2.235 2.449 2.664 2.878 3.093 3.307 3.522 3.736 3.951 4.165 4.380 4.594 4.809 5.023 5.238 5.452 5.667 5.881 6.096 6.310 6.525 6.739 6.954 7.168 7.383 7.598 7.812 8.027 8.241 8.456 8.670 8.885 9.099 9.314 9.528 9.743 9.957 10.172 10.386 10.601 10.815 11.030 11.244 11.459 11.673 11.888 12.102 12.317 12.531
- 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…mm 0.022 doidve of (41) bros Sibisconbydlo noitudo: M ILL 6. Classify each of the following as an Arrhenius acid (AA), a Arrhenius base (AB), a Bronsted-Lowry acid (BLA), a Bronsted-Lowry base (BLB), a Lewis acid (LA), and/or a Lewis base (LB). Select all that apply. Cact to nous dinoj Jusoraq silt ei ted You may need to draw the Lewis structure of some molecules to make this determination. The pKa of hydronium ion is -1.7. a. H₂O BLA LA BLB LB b. HI (pKa = -8) AA AB BLA BLB LA LB c. BH3 (pKa = ∞ BLA BLB LA LB d. NaOH AA AB BLA BLB LA LB e. CH3CH₂OH (pka = 16) AA BLA LA f. NC13 AA BLA LA AB BLB LB AB BLB LB g. NH3 (pKa = 39) AA AB BLA BLB LA LB h. F- AA BLA LA AB BLB LBI Normal 1 No Spac.. Heading 1 Heading 2 Title Styles Paragraph 5. Fill in the following table: [H3O"] РОН [OH'] ACID or BASE pH 7.21 9.84 x 10° M 3.25 2.64 x 102 M 2.49
- Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral Answer Bank H]= 1.0 x 10 pll=346 pOl - 541 OH |-26 x 10 pOll =831 pOll = 7.00 o|=98 x 10 " 1-63x 10 pll=10.38 I= 74 x 10 contectua help privecy polisy terma of uasGiven that pKa = 3.14 at 25 deg C for HNO2, what is the pH of 0.173 mol L-1 NaNO2(aq) at 25 \deg C? What is the equilibrium concentration of HNO2? pH = Number (Give your answer accurate to 2 decimal places.) [HNO2]eq = Number mol L-1 (Give your answer accurate to 2 signficant figures.)5. a) The Kw value that we normally use is for room temperature (25°C). Calculate the equilibrium H+ concentration and pH of pure, neutral water at 0.0°C (Kw= 1.14 x 10-15at 0.0°C) b) Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution.(Kb= 4.37 x 10-4at 25°C)
- (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 HOCI, HI, Nal, NaOCl Increasing pH of 0.15-M solution Drag and drop your selection from the following list to complete the answer: HOCI Nal NaOC1 HI b NH, CI, HCI, KCI, NH3 Increasing pH of 0.15-M solution Drag and drop your selection from the following list to complete the answer: NH, CI KCI NH3 HCICalculate the pH and the equilibrium concentrations of HC6H606 and C6H6О6²- in a 0.1820 M ascorbic acid solution, H₂C6H606 (aq). For H₂C6H606, Ka1 = 7.9x10-5 and Ka2 = 1.6x10-¹2 pH = [HC6H606]] = [C6H606²-] = ΣΣ