If a more concentrated initial solution bicarbonate was used in beaker C, would it require more or less bicarbonate to neutralize the acid? Why?
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If a more concentrated initial solution bicarbonate was used in beaker C, would it require more or less bicarbonate to neutralize the acid? Why?
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- If a less concentrated initial solution of socium bicarbonate was used in beaker C, would that solution require more or less bicarbonate to neutralize the acid? Why?What happened to the pH when the cola and borax solution was added to the water? ExplainA stock solution was diluted in two steps. In a first step, 0.5 ml was diluted with 9.6 mL buffer. In a second step, 0.5 mL from the first step was diluted with 9.6 mL of buffer. The concentration of the mixture of the second step was determined to be 0.24 mg/mL. What was the concentration of the stock solution?
- If a 250 ml solution of ethanol in water is prepared with 4 ml of absolute ethanol (100%), what is the dilution factor?What is the purpose of: A. The concentrated salt solution? B. adding isopropyl alcohol to the solution? Why does it need to be in low temperature?In excess of alkaloidal reagent, did the precipitate formed dissolve or not? What is the evidence for your answer?
- fill in the volumes required to make the various dilutions of Coomassie Blue and their respective concentrations. show sample calculations.Can the rate of hydrate formation be increased by hydroxide ion as well as by acid? Explain.If 10g of salt was mixed in 1L water. What percent solution will this be.
- Compounds such as the sugar trehalose are used as compatible solutes (i.e., water replacements) in desiccated organisms. What are the requirements for a substance that is to beused in this manner?What is the pH of the solution given the following information? Methyl orange = yellow Methyl red = yellow Bromothymol blue = green Note: use the provided reference table for color indicators below as a guide pH 5 pH 8 pH 7 pH 6A 25.00 mL sample of 0.320 M LIOH is titrated with 0.750 M HNO3 at 25 °C. Calculate the initial pH before any titrant is added. pH = Calculate the pH of the solution after 5.00 mL of the titrant is added. pH =