- Research article
- Open Access
- Open Peer Review
New chemolysis for urological calcium phosphate calculi – a study in vitro
- Zhang Xiang-bo†1, 2,
- Wang Zhi-ping†1, 2Email author,
- Duan Jian-min†2,
- Lu Jian-zhong2 and
- Ma Bao-liang2
© Xiang-bo et al; licensee BioMed Central Ltd. 2005
- Received: 06 December 2004
- Accepted: 22 May 2005
- Published: 22 May 2005
Advances in techniques have left very few indications for open surgical extraction of urinary stones currently. These advances notwithstanding, the search continues for medical approaches to urinary stone management. In this study, we perform an in vitro study analyzing the efficiency and prospect of two new complex solutions in urological calcium phosphate calculi dissolution.
Eighteen stones composed mainly of calcium phosphates were taken from patients who underwent kidney stone surgery. These stones were large enough (weight range 0.514–0.928 g) to be fragmented and matched equally into six groups. Chemolysis of phosphate stones was done with six different solvents and was repeated 3 times with 6 stones for each solution. At 24, 48 and 72 h, reduction in weight, percentage weight change, and dissolution rate; the dissolution rates at pH 5.0, 7.0 and 8.5 for each solution, using different cations (Na+, K+ or Ca2+), according to different dilutions (1:1, 1:2, 1:3, 1:4) of S1 and S2 were simultaneously determined.
Our data indicate that test solutions S1 and S2 are effective solvents in the chemolysis of calcium phosphate stones. At twice dilutions, these solutions are even more useful in the treatment of stone disease.
- Dissolution Rate
- Calcium Phosphate
- Shock Wave Lithotripsy
- Calcium Oxalate
- Extracorporeal Shock Wave Lithotripsy
The most important phosphate-containing calculi involved in urinary stone disease are carbonate apatite, brushite, and struvite. Overall, phosphate stones account for 12–20% of all urinary stones and rank first in the list of recurrent calculi . The most definitive therapy involving any type of phosphate stone is calculus removal by shock-wave lithotripsy, percutaneous stone removal, or open surgery (especially in children). However, while technologies have successfully treated patients with phosphate calculi, they are associated with injury to the urinary tissue and retained stone fragments have resulted in recurrences.
Stone dissolution through chemolysis remains an option for urologists even in the advent of more sophisticated modalities in the treatment of urolithiasis. Chemolysis via acidification of the urine and antibiotic therapy (especially for infection stones) are important adjuvant modalities for phosphate calculi therapy. Hitherto, a many solutions have been tested in the quest for more effective dissolution agents. The most effective solution among them is Renacidin (R), which is a buffer consisting mainly of citrate and gluconate [2–4]. These solutions are delivered directly into the kidney by ureteric catheter or percutaneous nephrostomy, and are successful in the dissolution of struvite. But the injury to urothelium restrains their wide use. So, solutions with more dissolution efficiency and less side effects are needed urgently and may be used widely. Our in vitro study was designed to evaluate the effectiveness of two new complex solutions (using D-gluconic acid-lactone, D-gluconic-acid and other ingredients which makes them different from R) in the chemolysis of calcium phosphate stones.
Stones specimen preparation
Chemical analysis of 18 stones for stone dissolution. There was a predominance of calcium phosphate in almost all the stones and calcium oxalate was less than 10%.
Mean chemical composition of 18 stones, showing that there was a predominance of calcium phosphate in almost all the stones and calcium oxalate was less than 10%.
Preparation of solvent
Molecular formulae and molecular weights of chemical drugs used in our experiment
D-Gluconic Acid Lactone
Potassium citrate, tribasic
Potassium phosphate, monobasic
1. Physiologic sodium chloride solution (Phys).
2. Artificial urine (Art, pH5.7, according to Griffith et al ) consisting of urea (25 g/L), sodium chloride (4.6 g/L), potassium-dihydrogen-phosphate (2.8 g/L), sodium sulfate (2.3 g/L), potassium chloride (1.6 g/L), ammonium chloride (1.0 g/L), calcium chloride dehydrate (0.1 g/L), sodium oxalate (0.05 g/L), and sodium citrate (0.01 g/L), dissolved in 1000 ml. distilled water.
3. 0.03 M disodium ethylenediaminetetraacetic acid buffered to pH 8.5 with triethanolamine (EDTA, pH 8.5)
4. 10% Renacidin (R, pH 3.9), consisting of citric acid (28.2 g), gluconic acid (5.0 g), calcium carbonate (1.0 g), magnesium bicarbonate (14.5 g), citrate magnesium (2.5 g), dissolved in 1000 ml. distilled water.
Concentrations of chemical drugs contained in S1 and S2
D-Gluconic Acid Lactone
Potassium citrate, tribasic
Calcium chloride, anhydrous
6. Test solution 1 (S1, pH 3.9), prepared using citric acid (18.0 g), citrate magnesium (1.0 g), calcium carbonate (0.5 g), magnesium carbonate (7.5 g), D-gluconic-acid (3.0 g), dissolved in 100 ml. distilled water, and processed as described for S2. The concentrations of these ingredients are shown in Table 4).
We also altered the pH of these solutions to 4, 5, 7, and 8.5 to test their effectiveness and added different cations (Na+, by adding 302.7 mmol/L citrate sodium 10 ml. into 100 ml. of the initial solution; K+, by adding 302.7 mmol/L citrate potassium 10 ml. into 100 ml. of the initial solution; Ca2+, by adding 454.5 mmol/L calcium chloride anhydrous 10 ml. into 100 ml. of the initial solution). S1 and S2 were formulated according to different dilutions (1:1, 1:2, 1:3, 1:4). The pH of these changed solutions had no detectable variation. After stones were immersed in these solvents for 24, 48 and 72 h, reduction in weight, percentage weight loss, and dissolution rate were determined. Results were analyzed using the Multiple Comparisons Test with the alpha set at 0.05. Stones remaining after the dissolution period were weighed (gm), and final weights were applied to the following formula:
The formula used to determine the dissolution rate was:
Every stone was placed in a vessel containing solvents, which were held at a constant temperature of 37? using a thermostat. Solvents were exchanged 2 times per day at 6 ml/100 mg per stone each time. The pH values were constantly controlled by a pH meter (Mettler Toledo 320-S, sensitivity 0.01). The weight of the calculus was measured continuously by Electronic Semi-micro-, Analytical and Precision Balances (Sartorius BP211D-OCE, sensitivity 0.01 mg) and documented online with a computer system (PC windows 486, Software Wedge for window, version 1.1). The analysis represents six stones for each experiment, repeated three independent times.
Mean weight and percentage weight decrease after 24 and 72 h between groups dissolved with 6 different solutions. Phys = physiologic sodium chloride solution, pH 7.0. Art = artificial urine, pH 5.7. EDTA = 0.03 M disodium EDTA+TEA, pH 8.5. R = renacidin, pH 4.0. S1 = citrate complex 1, pH 4.0. S2 = citrate complex 2, pH 3.9. ± s, a P < 0.01 vs R, S1 and S2.b P < 0.05 vs S1, S2.c P < 0.05 vs S1. n = 18 for each group. For statistics, see results section.
Weight loss (mg)
Percentage weight loss (%)
3.52 ± 0.73a
18.15 ± 13.15a
0.00 ± 0.00a
1.33 ± 1.53a
2.48 ± 0.37a
7.44 ± 1.9a
0.00 ± 0.00a
0.00 ± 0.00a
43.78 ± 6.23ab
153.6 ± 20.84ab
4.67 ± 2.08ab
19.00 ± 5.19ab
114.4 ± 8.92c
346.14 ± 26.56c
13 ± 1.35c
40.5 ± 3.67c
127 ± 23.09
408.11 ± 62.94
13.5 ± 2.76
44.4 ± 7.37
138.5 ± 31.09
439.5 ± 102.00
5.77 ± 1.29
52.1 ± 15.75
The addition of Na+, K+ or Ca2+ (302.7 mmol/L Sodium citrate 10 ml, 302.7 mmol /L Potassium citrate 10 ml or 454.5 mmol/L Calcium chloride dihydrate 10 ml into initial solution 100 ml, respectively) caused no significant change in dissolution rate.
Chemolysis is useful for eliminating cystine stones as well as for cases in which lithotripsy or endourology is considered to be difficult or risky. It proved to be a useful method for reducing staghorn stones before performing lithotripsy . The type of chemolytic solution is dependent upon the composition of the stone and must be regarded as an effective adjuvant treatment . Calcium phosphate can be dissolved with Suby or R, but the treatment is often tedious and time consuming. Calcium oxalate, the major urinary stone component, cannot be dissolved by these solutions. EDTA and other strong calcium chelators cannot be used because of their local toxicity. Certain enzymes can digest the organic matrix of the stone . The first attempts to dissolve calcium stones were done by Hellstrom and Albright in 1930. They used citric acid for phosphate calculi, but this proved irritating to tissues. Suby and Albright modified the solution by adding magnesium oxide and sodium carbonate (Suby's G solution) [9, 10] to reduce injury to the rabbit bladder mucosa even though adding this cation reduced the speed of dissolution of struvite Mg (NH4) PO4. A contradictory conclusion was been made by a Dutch study  that magnesium in R promotes stone dissolution by cation exchange with calcium in apatite .
Our S1 and S2 solutions were similar to R although actual formulas were different. First, we added D-gluconic acid-lactone or D-gluconic-acid as new chelators which bind with calcium well by their special trait. Second, we used new ingredients and ingredients at different weights. The higher density of our solutions than R may be one of the factors which enhanced stone dissolution rates, but it may prevented further dissolution. When diluted twice, the solutions may have gained more space to accommodate cations than the initial solutions and achieve better effectiveness (P < 0.05, S1 and S2 vs R). The further diluted solutions had a lower concentration suggesting that less ingredient took part in the reaction thus accounting for a lower dissolution rate. So, we think twice diluted S1 and S2 may be more useful than their initial solutions.
The dissolution of the majority of the stones in this study can be attributed on the basis of their reaction equation:
3Ca+2 + 2 Citrate→CaCitrate→Ca2+ + CaCitrate
The citrate in the solution binds with the calcium component of the stone producing calcium citrate, thus preventing crystallization. The dissolution process may be brought about by the combination of the above reaction.
As the solubility of calcium phosphate is very pH dependent, the acidification of the urine by the incorporation of citric acid produce a pH between 3.0–4.0, the ideal pH for dissolution as described by Albright et al [9, 10]. When the pH is elevated, the citrate will react with cations thus losing its effectiveness. On the other hand, excessive alkalization may lead to the formation of calcium phosphate calculi. Added minor quantities of cations (Na+, K+ or Ca2+) in S1 and S2 apparently causes no significant change to their dissolution rate.
The study has shown that solutions S1 and S2 can dissolve calcium phosphate stones effectively in vitro at a precise dilution of their chemical components. Based on these findings, it is suggested that S1 and S2 may become useful complements to modern techniques of stone fragmentation such as extracorporeal shock wave lithotripsy and percutaneous surgery. Their roles may be suited for the treatment of infectious stones with a CaOx content of less than 10%. However, their safety profiles should be further investigated in order to support their use in subsequent human trials.
We are indebted to Zhi-ping Wang, Professor and director of the institute of urinary, the 2nd Hospital of LanZhou University, for his help in conducting the study and for reviewing the manuscript. We thank Jian-min Duan, Jian-zhong Lu, Bao-liang Ma, staff at the institute of urinary, the 2nd Hospital of Lanzhou University, for generously supplying the room for our experiment.
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