I CAN ADJUST THE LEVEL OF PH ON MY WATER IONIZER. IS IT ACTUALLY SAFE OR DANGEREOUS TO DRINK WATER HIGHER THAN 9.5 PH LEVEL OR EVEN A 10.0 PH LEVEL?
125833
It's probably not the best thing for you as this can mess up your body chemistry if you're not used to this.  Nothing really horribly serious will happen though because your fluids are buffers.  A buffer is a solution which doesn't drastically change pH if an acid or base is added.  For example, your blood is a buffer solution.  On a daily basis you eat all sorts of acidic or basic things, but your insides need to be kept at a consistent pH.  Because buffer solutions don't change pH very much, your body can stay at a constant pH, and your organs won't fail.  I also think I heard that many cities have water with a pH of 9.
71137
It's not C.  An increase in pH makes a solution more alkaline, meaning less H+ in the fluids.\n\nI'm going to say A here because a rise in pH is associated with increased O2 binding to hemoglobin.
673419
True the higher the pH the lower the concentrations
603701
we know that pH is ranged from totally basic to totally acidic, with neutrality (water) being at pH=7; so just display a range from 0 to 14 and color code it (red for acid and blue for basic) and place your findings there (ie before and after situations of NaCl towards the pH of the solution). Also place analogies (ie. the results of the pH due to NaCl concentration of 10% is equivalent to household ammonia)\n\nWhen explaining something to a non-science person, visuals and analogies always helps.
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Sodium Error\nMore correctly called alkali ion error, sodium ion error\noccurs at high pH, where hydrogen ion concentration\nis very low in comparison to sodium ion concentration.\nThe sodium ion concentration can be so high relative\nto hydrogen ion contration that the electrode begins to\nrespond to the sodium ion. This results in a reading\nthat is lower than the actual pH. Depending on the pH\nglass formulation, this can occur as low as 10 pH.\nWhere accurate high pH readings are required, the\nupper pH limit of the pH electrode should be checked\nand a specially formulated, high pH electrode used if\nnecessary. Compared to sodium, lithium ions will produce\na larger error, while the effect of potassium ions\nis negligible.
534626
typical pH electrode life is expected to be one year from the date of manufacture for most warranty purposes. They do depend on application and application variances (i.e. how stable the solution being tested is.. amount of variance, temperature , etc). these factors all shorten electrode expected life. As far as having 10 year working electrodes.. i have heard of this, but I wouldnt count on the quality of these elctrodes over a wide pH range. They should be tested and verified. They are most likely indicating near correct pH in a vary stable solution and not very responsive over a large range ( in other words they're currently zeroed into reading correctly and wont if the solution varies a lot). The failure rate after 2 months maybe the case with electrodes that have been on a shelf for long periods beore being commissioned for use or less likely but I have seen it - a bad "batch" of electrodes you received from stock. Consult your supplier for support. If these are being used in low temperature conditions (under say 45 degrees F) you may require thermal compensation to read correctly over the 32-45 degree range.
456132
The concept of 1.5M hydrogen gas is rather odd, but, yes, you use the Nernst Equation.  Don't forget to convert the pH to a molarity of H+ ions.
64256
WOW, you are really doing an over kill if you just want to electrolisize water.\n\nPure water does not conduct electricity.  Water will only conduct when it has ions dissolved in it, the more ions, the better it will conduct.  Tap water does have a small concentration of ions in it,  not much, but enough to make it conduct when you pass 30 volts through it.\nTo increase the conductivity, as you know, you can add some type of electrolyte to the water (like table salt, NaCl).\n\nLet me take a step back right now.\nIf you were to break apart water into pure Hydrogen and Oxygen gas, this only requires a very small voltage, something around 1.5 volts or there abouts (I can look this number up if it is that important to you).  One you have obtained the minimum voltage, it is the current passing through the water the controls the speed of electrolysis.\nAll the voltage over the minimum is called the "over voltage".\n\nWhen you apply a greater voltage than is necesary to the water, you increase the likely hood of reducing/oxidizing things other than water.  Without going into too much detail about the chemistry of it all, you are producing Hydrogen gas at your cathode (-), but at the anode (+), you are probably not producing pure Oxygen, more likely it is Chlorine gas since the Cl- ion is easier to oxidize than the Oxygen in the water.  When you add NaCl to the water, you are only making it easier for it to produce Cl2 gas since it concentration increases.\nThe choice of electrolyte is important as it determines exactly what gasses you will be producing.  In this case, the Cl- ion from the salt is keeping you from making Oxygen gas.  Cl2 gas is very corrosive (not to mention deadly).\n\nThe type of electrode is also very important as some metals will corrode very easily during electrolysis while others are relaitively inert.  Carbon (graphite) and inert metals like platinum, gold and silver (<-- $$$) and popular choices for the anode which is prone to corrosion.  However, for the cathode, you have much greater latitude since the electrode is said to be protected by virture of its charge.\nPersonally, I use carbon-graphite electrodes because of their relative inexpensiveness, however, they do tend to errode over time and need replacing.  When the graphite electodes erode, they leave a fine black powder in suspention in the water which can be filtered out.\n\nLong story short, that slime is most likely the remnants of your electodes corroding away.  Have you noticed you anode betting corroded?\n\nWhat I would do if I were you,\n-switch to graphite electrodes\n-reduce the input voltage in the cell to less than 10 volts (ideally less than 5)\n-use a NaOH electrolye in DI water
291582
Your blood keeps its pH range stable.
163134
Monocube kind of has the right idea, but not really. The first thing you look at is the pH. Normal range is 7.35 - 7.45, with the absolute being 7.4. the lower the #, the more acidic it is, and the higher it is the more alkalotic. \n\nThe next thing you look at is the PaCO2. Normal = 35 - 45. When CO2 mixes w/ H20, you get carbonic acid, so increased PaCO2 will cause the pH to be more acidic (lower pH), decreased - more alkaline (higher pH).\n\nThen you look at the HCO3 level. Normal is 22-26. Bicarb is alkaline. The higher the bicarb level, the more alkaline (higher pH) and decreased bicarb = more acidic (lower ph).\n\nSo, lets make up a blood gas:\npH 7.28  PaCO2 74 HCO3 26 (we'll forget the other results for now & concentrate on this part)\n\nOk, so we see that the pH is low, so this is an acidic result. Now - what's causing it? The respiratory system, or the kidneys? Our CO2 (respiratory) is high, which means acidic. The bicarb is normal, so it is not a metabolic (kidney) problem. This is a respiratory acidosis.\n\n And you want to know about compensation...compensated means that it is a chronic problem. Something that has been going on for awhile, and the body has had time to fix the problem, and return the pH back to the normal level. \nThe example we have above is an acute problem. The bicarb level is normal. It takes at least 24 hours for the kidneys to try to compensate for a respiratory problem. This is an acute respiratory acidosis.\n\nIf we change the values - pH 7.33, same PaCO2 - 74, and HCO3 of 32, then we see that the kidneys have now started to fix the problem. Our pH is still acidic, still caused by a respiratory issue, but the bicarb is now elevated, so this is a partially compensated respiratory acidosis.\n\nOnce again, changing values to pH 7.37, PaCO2 74, HCO3 36. Now our pH is in the normal range. BUT, this is where people get messed up - you have to remember that the absolute normal is 7.40. This pH is on the acidic side, even though it is in the normal range. So then you look at the other values. the CO2 is very high, but so is the bicarb.\n I have seen Doctors and nurses who are unfamiliar with blood gas interpretation freak out on a gas like this. Is this patient in respiratory distress? NO! let me explain why. This is a compensated respiratory acidosis. The pH is back in the normal range! This is a typical blood gas for a COPD patient. This is where they "live". They retain CO2, their levels are always high, so the kidneys "compensate".\n\n If you have more questions, feel free to email me at mike.marlow@yahoo.com I hope this helps you.
496131
The concentration of H+ is 3.0 x 10^-4, so you know that the pH will be around 4.  What you need is a calculator that has a LOG button to convert the 0.0003 to an integer value.\n\nSo on your calculator you press the LOG button and then type in 0.0003 and then a ")" and press ENTER.  \n\nYou should get a result that says: -3.522878745 or so.  You need to round off to -3.5 and since pH is the NEGATIVE log of the hydrogen ion concentration you get rid of the minus.\n\nThe answer is 3.5.\n\n1x10^-3.5 is approximately equal to 0.0003.
665031
pH is a measure of the activity of hydrogen ions (H+) in a solution and, therefore, its acidity or alkalinity. For dilute solutions, however, it is convenient to substitute the activity of the hydrogen ions with the molarity (mol/L) of the hydrogen ions (however, this is not necessarily accurate at higher concentrations [1] [2]).\n\nIn aqueous systems, the hydrogen ion activity is dictated by the dissociation constant of water (Kw = 1.011 × 10−14 M2 at 25 °C) and interactions with other ions in solution. Due to this dissociation constant a neutral solution (hydrogen ion activity equals hydroxide ion activity) has a pH of approximately 7. Aqueous solutions with pH values lower than 7 are considered acidic, while pH values higher than 7 are considered alkaline.\n\nThe concept was introduced by S.P.L. Sørensen in 1909, and is purported to mean "pondus hydrogenii" in Latin.[3] However, most other sources attribute the name to the French term pouvoir hydrogène. [4] [5] [6] In English, pH can stand for "hydrogen power,"[4] [5] [6] "power of hydrogen," [7] [8] or "potential of hydrogen."[3] [9] [10] All of these terms are technically correct.\nThough a pH value has no unit, it is not an arbitrary scale; the number arises from a definition based on the activity of hydrogen ions in the solution.\n\nThe precise formula for calculating pH is:\n\n \naH+ denotes the activity of H+ ions, and is unitless.\n\nIn dilute solutions (such as tap water), the activity is approximately equal to the numeric value of the concentration of the H+ ion, denoted as [H+] (or more accurately written, [H3O+]), measured in moles per litre (also known as molarity). Therefore, it is often convenient to define pH as:\n\n \nFor both definitions, log10 denotes the base-10 logarithm, therefore pH defines a logarithmic scale of acidity. The straight bars, indicating absolute value, make pH a unit-less quantity. For example, if one makes a lemonade with a H+ concentration of 0.0050 moles per litre, its pH would be:\n\n \n \nA solution of pH = 8.2 will have an [H+] concentration of 10−8.2 mol/L, or about 6.31 × 10−9 mol/L. Thus, its hydrogen activity aH+ is around 6.31 × 10-9. A solution with an [H+] concentration of 4.5 × 10−4 mol/L will have a pH value of 3.35.\n\nIn solution at 25 °C, a pH of 7 indicates neutrality (i.e. the pH of pure water) because water naturally dissociates into H+ and OH− ions with equal concentrations of 1×10−7 mol/L. A lower pH value (for example pH 3) indicates increasing strength of acidity, and a higher pH value (for example pH 11) indicates increasing strength of alkalinity. Note, however, that pure water, when exposed to the atmosphere, will take in carbon dioxide, some of which reacts with water to form carbonic acid and H+, thereby lowering the pH to about 5.7.\n\nNeutral pH 25 °C at is not exactly 7. pH is an experimental value, so it has an associated error. Since the dissociation constant of water is (1.011±0.005)×1014, pH of water at 25 °C would be 6.998±0.001. The value is consistent, however, with neutral pH being 7.00 to two significant figures, which is near enough for most people to assume that it is exactly 7. The pH of water gets smaller with higher temperatures. For example, at 50 °C, pH of water is 6.55±0.01. This means that a diluted solution is neutral at 50 °C when its pH is around 6.55 and that a pH of 7.00 is basic.\n\nMost substances have a pH in the range 0 to 14, although extremely acidic or extremely basic substances may have pH less than 0 or greater than 14. An example is acid mine runoff, with a molar concentration of 3981 M and a pH = -3.6.\nThe Grand Peptide Families\nThese peptides are ribosomal peptides, usually with hormonal activity. All of these peptides are synthesized by cells as longer "propeptides" or "proproteins" and truncated prior to exiting the cell. They are released into the bloodstream where they perform
408529
That sounds incredibly ropy, the water will combine with other contents of your stocmach. the second that occurs, one thing the water isn't, is pure!!\n\nIt is true that drinking *any* reasonably clean water to great excess can cause problems because you start removing salts from your body when you urinate.\n\nLosing electrolyte due to drinking gallons of water in a short space of time (can easily be fatal) is totally different than blaming it on the water being "too pure".\n\nI think I would counter your lab workers comments by asking them how many seconds they feel it takes the water to reach your stomach. Then after they ave said "ooh, about 1 perhaps", then ask them if the water would still be pure - swimming around with dil Hcl and the remains of the mornings breakfast.\n\nThen remind them of the ultra-pure water leaching out the "nutrients".\n\nNutrients?   And where would these leached nutrients "go" ?  Would they be filtered out by the kidneys (retained) ?\n\nLOL I am going to have to stop now or I could write for ages on this and I really need to do a little more work!
99468
Maybe the HCl concentration is too high?  Pepsin is active at pH 2.5.  Also how do you know the 'fish sample' is actually being broken down by pepsin?
356090
Supposedly, micro combination pH electrodes can measure pH with as little as 10 microliters of sample.  I've never used one, so I can't tell you how accurate they are or how much they cost, but it might be worth looking into.
451404
It depends on your definition of "danger", "residue", and "use".  If the use was acid neutralization, the only danger would be the salt formed and its impact on rusting metal.  If the NaOH was not "used up", it will stay basic for years, the pH indicating the level of "danger".  The residues could be caustic, salt, or a salt from how it was used.  You have to test to see what it is or know the "use".
621361
check this link-- http://www.orgsyn.org/orgsyn/prep.asp?prep=cv6p0468.\n\ninstead of Me use Ph