kidney stones‚ calcium oxalate and calcium phosphate‚ we will focus on those two in the discussion of formation‚ treatment‚ and prevention. Calcium stones like calcium oxalate and calcium phosphate stones form when urine is “supersaturated with the constituent ions that comprise the stone” (Figge). This means‚ when urine is supersaturated with calcium and oxalate ion that type of stone is more likely to form. This supersaturation results from the ionic activity of Ca^(2+) and oxalate and Ca^(2+) and
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The equation for the reaction between a free calcium ion and an EDTA compound in pH of 10 is a 1:1 reaction which allows to see how many calcium ions were stabilized and therefore dissociated from the CaC2O4. This number of moles can then be multiplied by the molecular mass of CaC2O4 to find the initial weight of the ions that dissociated which
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age‚ neonatal hypoglycemia‚ erythrocytosis‚ and hyperbilirubinia. Composite morbidity was present in 59% of untreated GDM‚ 18% of treated GDM‚ and in 11% of nondiabetic subjects (Langer et al‚ 2005). The most common complication was macrosomia/LGA (long gestationa age) which affected 46% and 19% of the newborns from treated and untreated mothers with gestational diabetes‚ respectively. The incidence of fetal death was 5.4. 3.6 and 1.8 per 1000 in untreated‚ treated and nondiabetic mothers‚ respectively
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In liver the marker enzymes such as ALT and AST levels were recorded‚ whereas in kidney the levels of calcium‚ oxalate‚ phosphate‚ uric acid‚ creatinine‚ ALT and AST were conducted. The histopathological studies of kidney was also carried out. The values obtained in all the biochemical analyses of urine‚ serum‚ liver and kidney were presented and discussed below
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and mix it by inverting it. Record color change. To tube 3‚ add 5 drops of 1 M ammonium thiocyanate. Mix. Record color change. To tube 4‚ add 5drops of 1 M ammonia solution. Mix. Record color change. B. Calcium oxalate equilibrium Put 5 mL of .1 M calcium chloride and 5 mL of .1 M sodium oxalate into 6 inch test tube. Mix by stoppering and inverting. Equilibrium is established by formation of white precipitate. Add concentrated HCl. Shake after each drop. Record any changes. C. Cobalt chloride
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major stone compositions are calcium oxalate‚ calcium phosphate‚ magnesium ammonium phosphate (struvite)‚ uric acid‚ and cystine. Calcium–based stones are the most common‚ causing more than 75% of cases‚ and calcium oxalate is the most common type of stone overall. A rare but increasingly recognized cause of nephrolithiasis is the use of the protease inhibitor indinavir in treating HIV patients. Kidney Stone type | Population | Circumstances | Details | Calcium oxalate | 80% | when urine is acidic
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Lab: 5 Experiment:13 Pre-Lab The purpose of this experiment is to observe an equilibrium reaction counteracting changes to it’s system all in accordance to Le Chatelier’s principle. An equilibrium reaction can be pushed toward products or reactant based on changes in temperature or concentration. The reversibility of reaction will also be looked at. Pre-Lab questions 1. The concentrations of products and concentrations of reactants remain constant but both reactions
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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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product‚ increasing the limiting reactant‚ possibly‚ is the most effective. In this experiment we were able to calculate limiting reactants from the reaction of CaCl2. 2H2O + K2C2O4.H2O(aq). As a group‚ we obtained our salt mixture of calcium chloride and potassium oxalate‚ and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution‚ leaving the precipitate. Once the precipitate was dried overnight‚ it was weighed and
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Solubility product The Solubility product is related to SPARINGLY SOLUBLE SALTS ONLY!!!!! Examples are silver chloride‚ lead(II) chloride‚ calcium sulphate (in other words‚ it deals with salts commonly called insoluble salts) Consider a sparingly soluble salt MX Imagine the reaction that occurs when the solid is placed in water aMX (s) + H2O [pic] aMn+ (aq) + bXm- (aq) The equilibrium expression would be [Mn+]a [Xm-]b [MX]a [H2O]
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