rupture of membranes and was admitted with a blood pressure ranging in the 180’s for systolic and 100’s-110’s for diastolic. She also had increased amounts of protein in her urine which is a warning sign for renal damage. She was placed on magnesium sulfate to help treat her hypertension and as prophylaxis for seizures. She stated she was unaware of her blood pressure until she was admitted. She also stated she is very active and is involved in high school sports and coaching and was very surprised
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and to observe the effect of different concentrations of sucrose on the mass of a potato cell. Results for Part One suggested that the molecular weight of albumin and starch was too large to pass through the dialysis tube‚ but glucose and sodium sulfate molecules were small enough to pass through the dialysis tube. Also‚ a decrease in water weight occurred due the dialysis tube being placed in a hypertonic solution. Results for Par Two showed the potato cell having a molar concentration of 0.2734
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Water Testing Lab Conclusion In this lab‚ chemical tests were used to check for the presence of calcium‚ chloride‚ and sulfate ions in water samples. To do this‚ the testers started with five samples: a reference‚ a sample of only the chemical being tested for‚ a control‚ distilled water‚ two home water samples‚ and a school water sample. To test for the ions in the water‚ a chemical that would react with the ion and create a precipitate was added. If the precipitate was not easily visible‚ a
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The Carbon Cycle is a complex series of processes through which all of the carbon atoms in existence rotate. The same carbon atoms in your body today have been used in countless other molecules since time began. The wood burned just a few decades ago could have produced carbon dioxide which through photosynthesis became part of a plant. When you eat that plant‚ the same carbon from the wood which was burnt can become part of you. The carbon cycle is the great natural recycler of carbon atoms. Unfortunately
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produced at the anode‚ making it acidic and hydroxide ions were produced at the cathode‚ making it basic. Sodium sulfate was used because pure water doesn’t contain a high enough concentration of ions to produce a current; therefore‚ the sodium sulfate was acting as the salt bridge in the reaction. This processes was demonstrated in parts B and C as well; however‚ instead of the sodium sulfate acting as the salt bridge‚ potassium iodide was substituted in part B and potassium chloride in part C. In
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Unit 3 Chemistry: VCAA Practice Exam Questions 1 Question 3 (2010) A sample of the insecticide dichlorodiphenyltrichloroethane (DDT)‚ C14H9Cl5‚ was found to contain 0.120 g of carbon. What mass of chlorine was present in the sample? A. 0.127 g B. 0.355 g C. 0.994 g D. 1.01 g Question 10 (2009) The level of carbon dioxide in the air in a spacecraft can be controlled by passing the air through canisters containing lithium hydroxide‚ LiOH. In a laboratory trial‚ the air in a 5.00 L container
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the different ions. QUESTION If copper (II) sulfate when mixed with sodium carbonate at different quantities combine to form ions in definite ratios. HYPOTHESIS / PREDICTION I believe that the ions will combine in definite ratios due to the fact that the valance electrons will not be changing throughout any chemicals; consequently the ions must combine in definite ratios. EXPERIMENTAL DESIGN A technique is performed in which copper (II) sulfate and sodium carbonate are placed together in various
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Added heat (removes H2O) | none | solution becomes muddy black-ish | CuO (s)copper oxide | heated into small‚ black‚ metallic almost shards | Added sulfuric acid | H2SO4 (aq) | turns shards and liquid blue-ish color | CuSO4 (aq)copper sulfate | joins the sulfate after filtering | Added zinc | Zn (s) | small‚ orange‚ metallic shards form in blue
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Percent of Water Crystallization and the Chemical Formula of a Hydrate Aim: To determine the percent water of crystallization and the chemical formula of a hydrate Materials * 400 ML beaker * Glass rod * 3 to 5 grams of hydrated copper (II) sulfate CuSO4 (crushed) * Bunsen burner * Spatula * Heating pad * Clamp and stand * Electronic balance Procedures Refer to Lab sheet Observations 1. The powder seems to be very bright and shiny before any heating 2. The blue powder are
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nitrateAmmonium Nitrate How they are manufactured? Ammonium nitrate is made commercially by passing ammonia gas (NH3) and a water solution of nitric acid (HNO3) through a pipe. The ammonia combines with the nitric acid to form ammonium nitrate. The formula for this reaction can be written as NH3 + HNO3 → NH4NO3. Large amounts of heat are released during the reaction‚ so the pipe and supporting equipment must be very strong. The solution of ammonium nitrate in water is allowed to evaporate‚ leaving
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