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Calibration of pH Meter

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Introduction

Calibration of pH Meter Importing the concept of pH and the definition of pH - A measure of acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing more than 7 with increasing alkalinity and decreasing with increasing acidity of less than 7. The pH scale normally used ranges from 0 to 14). Certain chemical compounds release H + (hydrogen ions when in water) and other release OH - (hydroxide ions. The pH of a solution is the measurement of H+ or OH - in the solution exists. pH value of p (potential power) H (hydrogen, the logarithm of the reciprocal of the hydrogen ion concentration in gram atoms per litre. The pH scale is a logarithmic scale. ...read more.

Middle

Submerge the meter up to the cap line in the 7.0 calibration solution and adjust the screw labelled pH 7 on the top of the meter with a screwdriver until the meter reads 7.0. And rinsed the meter with distilled water and gently blot the end dry with a paper towel. Next, submerge the meter up to the cap line in the 4.0 calibration solution and adjust the screw labelled pH 4 on the top of the meter with a screwdriver until the meter reads 4.0. After calibrating the pH meter, I turned the meter off, replaced the cap, and discarded their calibration solution. I calibrated 0.25M and 1M of HCl to observe the accurate results from my practical experiment and the result I achieved are stated below in the table. ...read more.

Conclusion

Electrodes should be checked before use, and electrodes with low accuracy and precision are to be excluded from further use. If I not followed the addressed points below, I would have discovered an error. * Rinsing the electrodes with distilled water before placing in another solution. * Making sure the pH meter is up to date, e.g. Battery. * Stirring the solution in a circular motion with the pH meter. * Readings of pH or adjustment of the pH with the appropriate acid or base. * Allowing enough time for meter's reading to stabilise. A. The hydrogen ion concentration of a solution of pH 2.5 = 10-2.5 = 3.16�10-3 M B. The pH of 0.25M acid solution = -log (0.25) = 0.602pH C. The concentration of H+ ions in a solution of pH 1.0 pH = -log10 [H+] -1 = +log10 [H+] [H+] = 1�10-1 = 0.1M ...read more.

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