1. Which of the following will prevent the dissociation of AgCl, when also present in the solution? Hint: Recall and apply important equilibrium principles. A. KNO, B. NANO, C. NaCI D. NACH,COO
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- A. What two compounds would be best to use in preparing a pH 9.0 buffer solution? justify your answer. Assume you have the acids and the sodium salts of their conjugate bases available to you. Answer: The two compounds best fo preparing a buffer solution with a pH of 9.0 would be hydrocyanic (HCN) and phenol (HOc6H5) because their pKa values are 9.40 and 9.80 respectively making their pH levels the closest to 9. B. WHat mass ration of sodium to acid is needed to prepare this buffer? C. Can this buffer solution better resist pH changes from a string acid addition or strong base addition?The odor of fish is due primarily to amines, especially methylamine(CH3NH2). Fish is often served with a wedge oflemon, which contains citric acid. The amine and the acidreact forming a product with no odor, thereby makingthe less-than-fresh fish more appetizing. Calculate the equilibrium constant for the reaction of citric acid with methylamine, if only the firstproton of the citric acid (Ka1) is important in the neutralizationreaction.1. What is an alkaline acid? In general how we prepare an alkaline buffer? Explain with example and describe in “BULLET POINTS” with mechanism that how an alkaline Buffer can maintain its pH even after adding slight amount of acid or alkali from outside?
- How can we answer these questions? 1) What other methods could you have used to identify the unknown chemical? 2). What is/are the dominant species in solution at pH = 4.4? 3) Does the solution at pH = 4.9 constitute a buffer? What about at pH- 5.9? ExplainAmmonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?If enough of a monoprotic acid is dissolved in water to produce a 0.0124 M solution with a pH of 6.72, what is the equilibrium constant, p?a, for the acid? kindly consider the following when answering the question For weak acids that are so dilute or so weak that the pH of the solution lies between 6 and 7, the autoprotolysis of water must be taken into account when determining the p?a value. At equilibrium, there are four species in solution, the weak acid, HA, its conjugate, A−, H3O+, and OH−. Start by developing four equations that describe what is occurring in the solution at equilibrium.
- Acidified potassium bromate(V), KBrO3, reacts with hydrogen sulfide, H2S, to give a yellow solid and an orange solution. On shaking the solution with trichloroethane, the trichloroethane layer turned orange-red. (a) Suggest the identity of yellow solid and the orange solution. Describe the type of reaction taking place. (b) Construct a balanced equation for the reaction between KBrO3 and H2S. (C) BrO3- is the conjugate base of HBrO3. Draw the dot and cross structure of HBrO3. (d) HBr is a stronger acid than HCl. However, HBrO3 is a weaker acid than HCIO3. Explain the difference in acidities.Due to the pandemic Covid-19, the uses of hand sanitizers are very important among us. Predict and explain the colour of the solution and pH value when red cabbage indicator was added to the hand sanitizers.4 b) At pH 1.58, calculate the free [PO43-] when [PO43-]t = 22 mM. You can either solve 4 simultaneous equations to solve this problem for [H3PO4], [H2PO4-], [HPO42-] and [PO43-], or simply calculate the ratio of the two highest concentration species at the pH of the solution, and then calculate [PO43-] from those values. What are the two highest concentration species at pH 1.58?
- The pH of a 0.250 M hypoiodous (HOI) solution is 5.620.a. Write the relevant acid-base reaction.b. What is the concentration of ?+?c. What is the value of ???Really hoping for solutions since I’m having a hard time with this. Pls. skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced. A. What mass of NaCH3COO should be added to 1.00 L of 0.100 M CH3COOH to produce a solution with pH = 5.00? Assume that the volume remains 1.00 L. Include your analysis of the problem and assumptions if any. Make sure your final answer has correct significant figures. B. For another experiment, you will need a buffer at pH 5.2. Outline steps you will do to adjust the pH of the buffer you made in A to pH 5.2. Show your calculations.An alkaline solution was prepared with LiOH in such a way that 0.65 g dry LiOH was directly mixed with 0.6 M 650 mL LiOH solution and finally 350 mL more water was added to it. Find the final pH of the solution. You need to consider 100% dissociation of LiOH.