1. A concentrated phosphoricacid solution is 85.5% H3PO4 by mass and has a density of 1.69 g/mL at 25°C.

1. A concentrated phosphoricacid solution is 85.5% H3PO4 by mass and has a density of 1.69 g/mL at 25°C. What is the molarity of H3PO4? What is the mole fraction of urea, CO(NH2)2, in a solution prepa

1. A concentrated phosphoricacid solution is 85.5% H3PO4 by mass and has a density of 1.69 g/mL at 25°C. What is the molarity of H3PO4? What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 5.6 g of urea in 30.1 g of methanol, CH3OH? How will an understanding of this concept help you in your healthcare career?

2. Describe the blood hydrogen carbonate buffer system.

-What happens when blood acidity rises? Show the equation.

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-What happens when the blood becomes more alkaline? Show the equation.

-Distinguish between strong and weak acid. List some clinical uses of these acids and write equations for their dissociation in water.

-Did you find any of these to be a challenge? Why or why not?

Provide APA reference for each question

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