The pH of juice or wine is a measure of the strength and concentration of the dissociated acids present in that medium. It is calculated using the concentration of hydrogen ions in the formula pH = -log10[H+] and can be adjusted through the addition of acid or base.
The pH of juice or wine is important to know as it plays a critical role in many aspects of winemaking, in particular wine stability. Boulton et al. (1996) writes that pH influences microbiological stability, affects the equilibrium of tartrate salts, determines the effectiveness of sulfur dioxide and enzyme additions, influences the solubility of proteins and effectiveness of bentonite and affects red wine colour and oxidative and browning reactions.
Understanding the relationship between pH and sulfur dioxide (SO2) is critical. SO2 has both antioxidant and antimicrobial properties, making it an extremely effective preservative for wine. The amount of SO2 in the free form, and in particular the molecular form which determines the effectiveness of SO2’s anti-microbial activity, depends on the pH of the wine. The higher the pH, the less SO2 will be in the useful free form AND the less effective this free SO2 will be. Therefore, all other things being equal, at a higher pH not only will more SO2 need to be added to achieve the desired level of free SO2, but the concentration of free SO2 required to have the desired antioxidant and antimicrobial properties will in itself also be greater. So if the vintage delivers higher than typical pH values, it’s important to think about adjusting SO2 levels during storage.
Calibration of pH meters before use is very important, and during vintage this should be done at the beginning of every day. Analysing a standard to ensure the pH meter is giving the right results is also important. This is often done using pH 4.00 and pH 7.00 buffers. Common sources of errors in pH meters include protein build-up from analysing juice samples or switching from juice to wine without cleaning the electrode. At the AWRI, pH electrodes are stored in 10 g/L potassium chloride made up in pH 4.0 buffer solution when not in use, and a cleaning solution is also used at regular intervals to remove protein from the electrode tip.
Checking the pH calibration:
A simple solution of saturated potassium bitartrate (1% or 10 g/L) should give a pH of 3.56 ± 0.02 or the error of measurement. A 0.1M acetic acid solution has a pH of 2.90. A 0.01M acetic acid solution has a pH of 3.40.
Checking the titratable acidity calibration:
Pipette accurately 3 x 25 mL of 0.1M HCl into three beakers. The average figure should be within the acceptable range of 7.46-7.56.
Titrate a 5g/L tartaric acid check solution. The titre must lie within 4.8-5.2 mL.
Most pH meters do not correct for the temperature of the sample being analysed. This means that if a sample of juice or wine is at 10°C and the pH meter has been calibrated at 20°C, then there will be an error in this measurement. Samples MUST be the same temperature as the temperature at which the pH meter was calibrated.
Precipitation of potassium bitartrate is both influenced by, and has an influence on, the pH and titratable acidity of a wine. When wines with pH values below 3.65 are cold stabilised, the pH lowers as potassium bitartrate drops out and the titratable acidity (TA) decreases. This occurs because for every molecule of potassium bitartrate that forms and precipitates, one free hydrogen ion is formed (that had been attached to the tartrate in KHT). Alternatively, when KHT precipitation occurs in wines with pH values above 3.65, the pH will increase (while the TA still decreases), as one free hydrogen ion is removed from solution (due to its incorporation into KHT). The magnitude of the pH shift will vary depending on the amount of KHT that is removed during both fermentation and cold stabilisation. Further information on the potassium bitartrate equilibrium and changes in pH and TA due to KHT precipitation can be found here.
The pH of a wine or juice is a measure of the concentration of free hydrogen ions in solution, while the TA is a measure of the total amount of hydrogen ions. Based on these definitions, one might be tempted to think there is a relationship between the pH and the TA in juices and wines. Unfortunately, there is no direct or predictable relationship between pH and TA, and the same titratable acidity can be measured in different juices with either low pH or high pH. The pH is not correlated with the concentration of acids present, but is influenced by their ability to dissociate.
Is it best to adjust acidity to a pH or titratable acidity value? Of course, one would hope that the pH can be adjusted to the desired value and at the same time achieve the desired TA value. However, if the desired values of both parameters cannot be achieved, then preference should be given to the pH, particularly with musts. This is because pH plays an important role in many aspects of winemaking and wine stability. The pH influences microbiological stability, affects the equilibrium of the tartrate salts, determines the effectiveness of sulfur dioxide and enzyme additions, influences the solubility of proteins and effectiveness of bentonite and affects red wine colour and oxidative and browning reactions (Boulton et al. 1996).
It is best to adjust the acid as early as possible because juice and wine are more stable at lower pH. In the case of red musts, it is advisable to adjust the pH to 3.4 or lower. If the desirable TA cannot be achieved, then the must should be adjusted to pH 3.4 regardless of the amount of tartaric acid required to do so. Note that a large amount of the added acid will precipitate later as KHT, resulting in a decrease in the TA. Given that the pH of red wines is likely to rise during fermentation, due to the leaching of potassium ions from the skins, it is recommended that the pH be measured during fermentation on skins and that additions be made to maintain the pH in the range 3.4 – 3.5.
If all the individual acids in a wine are expressed as tartaric acid equivalents and summed, the value for the total acid concentration will be greater than the value for the titratable acidity concentration. This is because the total acidity is the sum of all the organic acid anions in solution, while the titratable acidity measures the total available hydrogen ions in solution. The titratable acidity will always be less than would be expected from the organic acid concentration (Boulton et al.1996). This is because total acidity analysis measures both the dissociated and undissociated forms of each individual acid. As an example, if a solution of 1 g/L tartrate, as KHT, is analysed for titratable acidity, the result will be 0.5 g/L expressed as tartaric acid. However, if the solution is analysed for total acidity, using HPLC for example, the result will be 1 g/L as tartrate.
Winemakers are generally used to observing TA decreases during fermentation due to the precipitation of potassium bitartrate (KHT), which becomes less soluble with increasing ethanol concentration. When the KHT precipitates, it removes a proton from solution that would otherwise have contributed to the TA concentration. Winemakers are generally less used, however, to increases in TA during fermentation. When TA increases are observed, they are almost always associated with red wine ferments. Given it is difficult to obtain a homogeneous sample of red must immediately after crushing, inaccurate must titratable acidity results can sometimes explain TA discrepancies. Analytical error might also explain TA variations in some cases, while errors in tartaric acid additions due to inaccurate weighing might explain the results in others. If analytical error and other factors, such as a high acetic acid concentration can be ruled out, then increases in TA can often be attributed to increased concentrations of succinic acid.
Succinic acid is a normal by-product of alcoholic fermentation and its mean concentration in red and white Australian wines is in the order of 1.2 g/L and 0.6 g/L, respectively. However, concentrations as high as 3.0 g/L have been recorded in red wines for which TA increases have been observed (AWRI publication #817). Yeast strain appears to be an important variable affecting the amount of succinic acid produced. However, a number of other factors might also influence the production of succinic acid, including fermentation temperature, aeration, must clarity and composition (e.g. sugar concentration, nutrient content, pH, titratable acidity, presence of excess SO2), and other environmental factors (AWRI publication #817). It is not currently possible to predict with certainty whether a fermentation will produce a higher than usual amount of succinic acid. However, selection of a known high succinic acid producing yeast strain, used in combination with several of the factors mentioned above, will increase the chance of increased TA.
Boulton, R.B.; Singleton, V.L.; Bisson, L.F.; Kunkee, R.E. 1996. Principles and practices of winemaking. New York: Chapman & Hall: 521–253.
Coulter, A.D.; Godden, P.W.; Pretorius, I.S. 2004. Succinic acid—How it is formed, what is its effect on titratable acidity, and what factors influence its concentration in wine? Aust. N.Z. Wine Ind. J. 19(6): 16–20, 22–25.