Calculate the pH at 25 °C of a 0.62 M solution of lidocaine HCI (C₁4H₂, NONH,CI). Note that lidocaine (C₁4H₂NONH) is a weak base with a pk of 7.94. Round your answer to I decimal place.

A solution is prepared at 25 °C that is initially 0.35M in nitrous acid (HNO2), a weak acid with K = 4.5 × 10 4, and 1.2M in potassium nitrite (KNO2). Calculate the pH of the solution. Round your answer to 2 decimal places. pH=0

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…

Calculate 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