Kidney stones are a common ailment affecting approximately 10% of adults in the United States. They form when solutes precipitate out of solution as crystals in the urinary tract, and they can cause severe pain in the side, back, abdomen, and groin. Individuals who have been previously diagnosed with kidney stones have an increased probability of developing new stones relative to unaffected individuals. Different measures may help prevent the formation of different kinds of stones, so analysis of the composition of stones that have been passed or removed can aid in preventing recurrence. Stones can be ground into fine powders, dissolved in a small amount of solvent, and analyzed by infrared (IR) spectroscopy, as shown in Figure 1.Figure 1 Schematic of kidney stone analysis by IR spectroscopyIR analysis of kidney stones from 50 individuals revealed the percentage of stones that contain each component, shown in Table 1 along with solubility data.Table 1 Kidney Stone Composition ParametersSome studies indicate that potassium citrate, taken orally, may prevent the formation of calcium oxalate crystals, the most abundant component of kidney stones. Oxalic acid, shown in Figure 2, is significantly more soluble than calcium oxalate.Figure 2 Structure of oxalic acid and its associated anions with increasing pHPotassium citrate alkalinizes the urine, potentially causing a decrease in oxalate solubility and the formation of more crystals. However, potassium citrate can also react with calcium oxalate according to the unbalanced equation shown in Reaction 1:CaC2O4 + K3(C6H5O7) → Ca3(C6H5O7)2 + K2C2O4Reaction 1Calcium citrate and potassium oxalate are both hundreds of times more soluble than calcium oxalate, so the presence of citrate and potassium ions can help maintain calcium and oxalate ions in solution. This effect may be sufficient to overcome the decreased solubility that occurs at higher pH levels.Adapted from Primiano A, Persichilli S, Gambaro G, et al. FT-IR analysis of urinary stones: a helpful tool for clinician comparison with the chemical spot test. Dis Markers. 2014;2014:176165. Question 7Given the unbalanced equation (Reaction 1) and the molecular weight of calcium citrate (498.5 ng/nmol), if 15 nmol of calcium oxalate is mixed with 15 nmol of potassium citrate, what is the approximate theoretical yield of calcium citrate?A.1,250 ngB.2,500 ngC.3,750 ngD.7,500 ngSubmit
Question
Kidney stones are a common ailment affecting approximately 10% of adults in the United States. They form when solutes precipitate out of solution as crystals in the urinary tract, and they can cause severe pain in the side, back, abdomen, and groin. Individuals who have been previously diagnosed with kidney stones have an increased probability of developing new stones relative to unaffected individuals. Different measures may help prevent the formation of different kinds of stones, so analysis of the composition of stones that have been passed or removed can aid in preventing recurrence. Stones can be ground into fine powders, dissolved in a small amount of solvent, and analyzed by infrared (IR) spectroscopy, as shown in Figure 1.Figure 1 Schematic of kidney stone analysis by IR spectroscopyIR analysis of kidney stones from 50 individuals revealed the percentage of stones that contain each component, shown in Table 1 along with solubility data.Table 1 Kidney Stone Composition ParametersSome studies indicate that potassium citrate, taken orally, may prevent the formation of calcium oxalate crystals, the most abundant component of kidney stones. Oxalic acid, shown in Figure 2, is significantly more soluble than calcium oxalate.Figure 2 Structure of oxalic acid and its associated anions with increasing pHPotassium citrate alkalinizes the urine, potentially causing a decrease in oxalate solubility and the formation of more crystals. However, potassium citrate can also react with calcium oxalate according to the unbalanced equation shown in Reaction 1:CaC2O4 + K3(C6H5O7) → Ca3(C6H5O7)2 + K2C2O4Reaction 1Calcium citrate and potassium oxalate are both hundreds of times more soluble than calcium oxalate, so the presence of citrate and potassium ions can help maintain calcium and oxalate ions in solution. This effect may be sufficient to overcome the decreased solubility that occurs at higher pH levels.Adapted from Primiano A, Persichilli S, Gambaro G, et al. FT-IR analysis of urinary stones: a helpful tool for clinician comparison with the chemical spot test. Dis Markers. 2014;2014:176165. Question 7Given the unbalanced equation (Reaction 1) and the molecular weight of calcium citrate (498.5 ng/nmol), if 15 nmol of calcium oxalate is mixed with 15 nmol of potassium citrate, what is the approximate theoretical yield of calcium citrate?A.1,250 ngB.2,500 ngC.3,750 ngD.7,500 ngSubmit
Solution
To calculate the theoretical yield of calcium citrate, we need to balance the equation first. The balanced equation is:
CaC2O4 + 3K3(C6H5O7) → 2Ca3(C6H5O7)2 + 3K2C2O4
From the balanced equation, we can see that one mole of calcium oxalate reacts with three moles of potassium citrate to produce two moles of calcium citrate.
However, in the question, we are given that 15 nmol of calcium oxalate is mixed with 15 nmol of potassium citrate. This means that not all of the calcium oxalate will react because there is not enough potassium citrate.
Therefore, the reaction will be limited by the amount of potassium citrate, and only 5 nmol of calcium oxalate will react to produce 10 nmol of calcium citrate.
The molecular weight of calcium citrate is given as 498.5 ng/nmol. Therefore, the theoretical yield of calcium citrate can be calculated as follows:
10 nmol * 498.5 ng/nmol = 4,985 ng
However, this answer is not in the options. The closest option is 5,000 ng, but it's not listed. There might be a mistake in the question or the options.
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