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Which of the following are typically TRUE of an oxidizing agent? 1. It causes oxidation. 2. It gains electron(s). 3. It is the reduced substance. 4. all 5. none
What volume of 0.25 M HNO3 (aq) reacts with 4.8 ml of 0.150 M Na2CO3 (aq) when the two solutions are mixed?please show work step by step.
Calculate the pH of the solution after the addition of 30ml of 0.1M NaOH. Show you work. Draw the structure of the form is His predominating in solution at neutral pH.
A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produced the following data: Volume of O2 produced at room conditions
125 mole of oxygen gas is added to carbon in a .25L container. The mixture equilibriates at 500K. Calculate the equilibrium concentration of carbon monoxide, knowing that K=.086 at 500K.
Methyl salicylate + NaOH --> disodium salicylate + Ch3OH + H20 disodium salicylate + H2SO4 --> salicylic acid + Na2SO4 The two chemical equations above are for the synthesis of salicylic acid. In the second equation, when H2SO4 is added quickly to..
Calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH = 10.10 [CH3NH2]/[CH3NH3CL] = ? I know that the answer is 0.34 but is not wright to write it in this way in mastering chemistry and they are errors in the submission
A 20.00 mL sample of 0.1026 M HCl was titrated with NaOH solution. The initial buret reading was 0.25 mL, and the final reading was 18.78 mL.
Consider a mixture of salt NaA and weak acid HA. Please derive the pH Henderson Hasselback equation by writing the equilibrium expression. Define the pKa
Why is the first step in an electrophilic aromatic bromination reaction so much more endothermic than the first step in an electrophilic addition to an alkene
A mixture of 40 Ml of methyl butyrate (MW-102.1 g/mol,d-0.89 g/mL) and 10 mL butyric acid (MW=88.1 g/mol, d=0.96 g/ML) is distilled.
Calculate the of the following solutions and report it to the correct number of significant figures: Seawater with H3O = 7.0×10?9
Calculate the [H3O+] and the pH for a buffer that consists of 0.13 M HF and 0.29 M KF. (Ka of HF = 6.8x10^-4)
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